Ever wonder how a mass amount such as moles can be converted into the volume amount of liters? Well, molarity serves as the bridge between moles and liters.

Concept #1: Definition of Molarity

Anytime that you hear the term **molarity **used, just think that we are talking about how many moles of a **solute** are in a liter of **solution**.

Forgot what's the difference between a solute and a solution? Here's a reminder:

Concept #2: The difference between a solute and solvent

In a **homogeneous mixture**, the smaller amount is the **solute**, and the larger amount is the **solvent**. When dissolving a solute into a solvent they make a solution.

Example #1: 2.64 grams of an unknown compound was dissolved in water to yield 150 mL of solution. The concentration of the solution was 0.075 M. What was the molecular weight of the substance?

A **concentrated solution** can become a **diluted solution** with the addition of water.

Example #2: A solution is prepared by dissolving 0.1408 mol calcium nitrate, Ca(NO_{3})_{2}, in enough water to make 100.0 mL of stock solution. If 20.0 mL of this solution is then mixed with an additional 90 mL of deionized water, calculate the concentration of the calcium nitrate solution.

We know how to calculate the molarity of a compound, but what do we do when we need the *molarity of ions *within the compound? Let's see.

Practice: What is the molarity of calcium ions of a 650 mL solution containing 42.7 g of calcium phosphate?

Now let's try connecting molarity with an equation from the past, density.

Practice: A solution with a final volume of 750.0 mL was prepared by dissolving 30.00 mL of benzene (C6H6, density = 0.8787 g/mL ) in dichloromethane. Calculate the molarity of benzene in the solution.

Determine the molarity of a solution formed by dissolving 0.468 g of MgI 2 in enough water to yield 50.0 mL of solution.
A. 0.0287 M
B. 0.0107 M
C. 0.0936 M
D. 0.0337 M
E. 0.0651 M

How many moles of Nal are in 23.0 mL of a 0.250 M solution?
A. 0.250 moles Nal
B. 5.75 moles Nal
C. 0.00575 moles Nal
D. 0.0920 moles Nal
E. 10.9 moles Nal

What mass of KBr is needed to make a 6.54 M solution in 25.00 mL ?
A. 19.5 g
B. 1.37 g
C. 0.151 g
D. 1.95 x 104 g

How many grams of phosphoric acid are there in 175 mL of a 3.5 M solution of phosphoric acid (MW 98.00 g/mol)?
a) 0.61 g
b) 60 g
c) 21 g
d) 4.9 g
e) 610 g

Which diagram represents the most concentrated solution?

What is the molarity of a solution made by dissolving 8.56 g of sodium in acetate water and diluting to 750.0 mL?
(A) 5.30 M
(B) 0.139 M
(C) 0.104 M
(D) 0.0783 M

Determine the mass (g) of solute required to form 25 mL of a 0.1881 M H 2O2 solution.
a) 0.031
b) 160
c) 0.31
d) 0.022
e) 0.16

How many moles of PO43– ions are in 2.00 L of a 0.600 M solution of a Ca 3(PO4)2?
a) 0.600
b) 1.000
c) 1.200
d) 2.400
e) 3.600

How many milliliters of a 0.184 M NaNO 3 solution contain 0.113 moles of NaNO3?
a. 885 mL
b. 614 mL
c. 326 mL
d. 163 mL
e. 20.8 mL

3.25 g of acetone (CH 3COCH3, 58.08 g/mol) are dissolved in water to make 125.00 mL of a solution. What is the molarity of the acetone?
a. 0.0560 M
b. 0.448 M
c. 0.560 M
d. 0.000448 M
e. Cannot be calculated from the information given.

How many chloride ions are present in 65.5 mL of 0.210 M AlCl3 solution?
a. 4.02 x 1023 chloride ions
b. 5.79 x 1024 chloride ions
c. 2.49 x 1022 chloride ions
d. 8.28 x 1021 chloride ions
e. 1.21 x 1022 chloride ions

If 4.49 g NaNO3 (molar mass = 85.0 g/mol) is dissolved in enough water to make 250.0 mL of solution, what is the molarity of the sodium nitrate solution?
a. 0.0180 M
b. 0.0528 M
c. 0.211 M
d. 0.0132 M
e. 18.0 M

If 5.15 g Fe(NO3)3 (molar mass = 241.9 g/mol) is dissolved in enough water to make exactly 150.0 mL of solution, what is the molar concentration of nitrate ion?
a. 0.0473 M
b. 0.0212 M
c. 0.142 M
d. 0.318 M
e. 0.426 M

What is the mass of potassium iodide (molar mass = 166.0 g/mol) in 50.0 mL of 5.75 x 10–2 M KI (aq)?
a. 288 g
b. 0.191 g
c. 0.00288 g
d. 0.477 g
e. 191 g

How many milligrams of NaCN are required to prepare 712 mL of 0.250 M NaCN?

What volume (in µL) of 0.100 M HBr contains 0.170 moles of HBr?

How many moles of Ca2+ ions are in 0.100 L of a 0.450 M solution of Ca3(PO4)2?

Which of the following solutions will have the highest concentration of bromide ions?
a) 0.10 M NaBr
b) 0.10 M CaBr2
c) 0.10 M AlBr3
d) 0.05 M MnBr4
e) All of these solutions have the same concentration of bromide ions.

Calculate the molarity of bromide ions in a solution if you mixed 12.86 g calcium bromide, CaBr2, in enough water to make 305.0 mL of solution

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.
A) 1.50 M
B) 1.18 M
C) 0.130 M
D) 0.768 M
E) 2.30 M

A 4.691 g sample of MgCl2 is dissolved in enough water to give 750 mL of solution. What is the magnesium ion concentration in this solution?
A) 3.70 x 10–2 M
B) 1.05 x 10–2 M
C) 6.57 x 10–2 M
D) 4.93 x 10–2 M
E) 0.131 M

How many grams of KMnO 4 are required to prepare 750.0 mL of a 0.125 M solution?
A. 11.4
B. 14.8
C. 15.2
D. 17.5
E. 27.5

Hydrochloric acid is widely used as a laboratory reagent, in refining ore for the production of tin and tantalum, and as a catalyst in organic reactions. Calculate the number of moles of HCl in 62.50 mL of 0.500 M hydrochloric acid.
(A) 0.03125 mol
(B) 0.125 mol
(C) 8 mol
(D) 31.25 mol
(E) 125 mol

How many liters of a 0.0550 M NaOH solution contain 0.163 moles of NaOH?
a) 3.37 L
b) 1.48 L
c) 8.97 L
d) 2.96 L
e) 1.12 L

What is the molarity of formaldehyde in a solution containing 0.30 g of formaldehyde (CH2O) per mL?
(A) 0.3 M
(B) 1 M
(C) 3 M
(D) 10 M
(E) 30 M

An aqueous solution that is 42.0% of C 2H6 by mass has a density of 1.78 g/mL. What is the molarity of this solution?
a. 24.9 M
b. 0.0249 M
c. 1.40 M
d. 43.0 M
e. 0.052 M

What is the molarity of an NaOH solution which contains 24.0g of NaOH dissolved in 200mL of solution?

What is the molarity of formaldehyde in a solution containing 0.300 g of formaldehyde (CH2O) per mL?
(A) 0.0000100 M
(B) 0.0100 M
(C) 0.100 M
(D) 1.00 M
(E) 10.0 M

How many grams of KOH are required to prepare a 250.0 mL solution of 0.50 M KOH? (K = 39.10 amu, O = 16.00 amu, H = 1.008 amu)
a. 16 g
b. 13 g
c. 11 g
d. 9.0 g
e. 7.0 g

A solution has 25.65 g of calcium perchlorate (MW = 238.98 g/mol) in 1.23 L. What is the concentration of perchlorate ions in M? Enter your answer with 3 decimal places and no units.

Calculate the number of moles HCl in 62.85mL of 0.453 M hydrochloric acid.

A 46.2-mL, 0.568 M calcium nitrate [Ca(NO3)2] solution is mixed with 80.5 mL of 1.396 M calcium nitrate solution. Calculate the concentration of the final solution.

What would be the molarity of NaOH in a solution made by dissolving 57.2 g of NaOH in enough water to make a final volume of exactly 500 mL? The molar mass of NaOH is 40.01 g/mol?
A. 6.99 M
B. 14.3 M
C. 2.86 M
D. 5.71 M
E. 0.1092 M

Which one of the following solutions will have the greatest concentration of hydroxide ions?
a) 0.100 M hydrochloric acid
b) 0.100 M magnesium hydroxide
c) 0.100 M ammonia
d) 0.300 M rubidium hydroxide
e) 0.250 M calcium hydroxide

How many milliliters of a 6.00 M
NaOH solution are needed to provide 0.355 mol of NaOH?

You may want to reference (Pages 152 - 157) Section 4.4 while completing this problem.What volume, in milliliters, of a 0.150 M solution of KCl contains 2.55 g of the compound?

You may want to reference(Pages 144 - 148)Section 4.5 while completing this problem.How many milliliters of 6.1 M
HCl solution are needed to obtain 0.16 mol of HCl?

You may want to reference (Pages 152 - 157) Section 4.4 while completing this problem.
What volume of 0.220 M ethanol solution contains each of the following number of moles of ethanol?0.46 mol ethanol

You may want to reference (Pages 152 - 157) Section 4.4 while completing this problem.
What volume of 0.220 M ethanol solution contains each of the following number of moles of ethanol?1.23 mol ethanol

You may want to reference (Pages 152 - 157) Section 4.4 while completing this problem.
What volume of 0.220 M ethanol solution contains each of the following number of moles of ethanol?1.3×10−2 mol ethanol

Neurotransmitters are molecules that are released by nerve
cells to other cells in our bodies, and are needed for muscle
motion, thinking, feeling, and memory. Dopamine is a common neurotransmitter in the human brain.
Experiments with
rats show that if rats are dosed with 3.0 mg/kg
of cocaine
(that is, 3.0 mg
cocaine per kg of animal mass), the concentration of dopamine in their brains increases by 0.75 M after 60 seconds. Calculate how many molecules of dopamine
would be produced in a rat (average brain volume 5.00 mm3)
after 60 seconds of a 3.0 mg/kg
dose of cocaine.

A medical lab is testing a new anticancer drug on cancer cells.
The drug stock solution concentration is
1.5 10-9 M, and
1.00
mL
of this solution will be delivered to a dish containing
2.0 105
cancer cells in 5.00 mL
of aqueous fluid.What is the
ratio of drug molecules to the number of cancer cells in the
dish?

How many grams of ethanol, CH3CH2OH, should you dissolve in water to make 1.00 L of vodka (which is an aqueous solution that is 6.86 M ethanol)?

You want to analyze a silver nitrate solution.Given that a 0.160 M
HCl(aq) solution costs $39.95 for 500 mL, and that KCl costs
$10/ton, which analysis procedure is more cost-effective?

How much dry solute would you take to prepare each of the following solutions from the dry solute and the solvent?126 mL of 0.505 M
KCl

How much dry solute would you take to prepare each of the following solutions from the dry solute and the solvent?126 mL of 0.115 M
NaNO3

You may want to reference (Page 153) Section 4.4 while completing this problem.What mass (in grams) of Mg(NO3)2 is present in 145
mL of a 0.150
M solution of Mg(NO3)2?

Calculate the number of moles of solute present in each of the following aqueous solutions.700 mL of 0.260 M
SrBr2

Describe how you would prepare each of the following aqueous solutions, starting with solid KBr.0.80 L of 1.6×10−2 M
KBr

The average adult human male has a total blood volume of 4.8 L .If the concentration of sodium ion in this average individual is 0.136
M, what is the mass of sodium ion circulating in the blood?

You may want to reference (Pages 542 - 552) Section 13.5 while completing this problem.Calculate the number of moles of solute present in 255
mL of 1.60
M HNO3(aq).

A person suffering from hyponatremia has a sodium ion concentration in the blood of 0.116
M and a total blood volume of 4.8 L .What mass of sodium chloride would need to be added to the blood to bring the sodium ion concentration up to 0.138
M, assuming no change in blood volume?

The average adult male has a total blood volume of 5.0 L. After drinking a few beers, he has a BAC of 0.22. Blood alcohol concentration (BAC), is given in units of grams of alcohol per 100 mL of blood.What mass of alcohol is circulating in his blood?

Describe how you would prepare each of the following aqueous solutions.
You may want to reference (Pages 539 - 541)Section 13.4 while completing this problem.Give the mass of the solute and the volume of the solvent for 1.60
L of 0.130
M (NH4 )2 SO4 solution, starting with solid (NH4 )2 SO4.

Which will contain the greater number of moles of potassium ion: 30.0 mL of 0.15 M
K2CrO4 or 25.0 mL of 0.080 M
K3PO4?

You may want to reference (Pages 152 - 157) Section 4.4 while completing this problem.How many grams of sucrose (C12H22O11) are in 1.50 L of a 0.771 M sucrose solution?

How many
moles of protons are present in 36.0 mL of a 4.50 M solution of nitric acid?

You may want to reference (Pages 152 - 157) Section 4.4 while completing this problem.What mass of KBr (in grams) should you use to make 350.0 mL of a 1.60 M solution of KBr?

You may want to reference(Pages 144 - 148)Section 4.5 while completing this problem.How many moles of KBr are present in 160. mL of a 0.117 M solution?

How many moles of KCl are contained in each of the following?0.557 L of a 2.3 M
KCl solution

How many moles of KCl are contained in each of the following?1.7 L of a 0.86 M
KCl solution

How many moles of KCl are contained in each of the following?120 mL of a 1.81 M
KCl solution

A laboratory procedure calls for making 410.0 mL of a 1.2 M NaNO3 solution.What mass of NaNO3 (in g) is needed?

A chemist wants to make 6.0 L of a 0.310 M CaCl2 solution.What mass of CaCl2 (in g) should the chemist use?

Write a detailed set of instructions for making two solutions: (1)
100 mL
of
16
MNaOH
from solid sodium hydroxide and (2)
1.00 L
of 0.1 M NaOH
from your first solution. You have in your
lab: volumetric flasks marked to contain 100.0 mL
and 1.000 L,
a graduated cylinder, and a balance.Calculate the mass of solid sodium hydroxide needed for making a 100 mL
solution of
16
MNaOH.

Neurotransmitters are molecules that are released by nerve
cells to other cells in our bodies, and are needed for muscle
motion, thinking, feeling, and memory. Dopamine is a common neurotransmitter in the human brain.
Patients with Parkinsons
disease suffer from a shortage of dopamine and may need to
take it to reduce symptoms. An IV (intravenous fluid) bag is
filled with a solution that contains 400.0 mg dopamine per
250.0 mL of solution. What is the concentration of dopamine in the IV bag in units of molarity?

Ritalin is the trade name of a drug, methylphenidate, used
to treat attention-deficit/hyperactivity disorder in young
adults. The chemical structure of methylphenidate is shown in the figure below.
A tablet contains a
35.0-mg
dose of Ritalin. Assuming all the drug ends up in the bloodstream,
and the average man has a total blood volume of 5.0 L,
calculate the initial molarity of Ritalin in a mans bloodstream.

Ritalin is the trade name of a drug, methylphenidate, used
to treat attention-deficit/hyperactivity disorder in young
adults. The chemical structure of methylphenidate is shown in the figure below.
Ritalin has a half-life of 3 hours in the blood,
which means that after 3 hours the concentration in the
blood has decreased by half of its initial value. For the
man in Part B, what is the concentration of Ritalin in
his blood after 6 hours?

An aqueous NaCl solution is made using 126 g of NaCl diluted to a total solution volume of 1.15 L .Calculate the molarity of the solution.

One cup of fresh orange juice contains 124
mg of ascorbic
acid (vitamin C, C6H8O6).
You may want to reference (Pages 145 - 148) Section 4.5 while completing this problem.Given that one cup = 237.2
mL, calculate the molarity of vitamin C in orange juice.

Calculate the molarity of the following aqueous solutions.0.550 g Mg(NO3 )2 in 250.0 mL of solution

Calculate the molarity of the following aqueous solutions.22.5 g LiClO4 3H2 O in 125 mL of solution

You may want to reference (Page 151) Section 4.4 while completing this problem.What is the molarity of a solution containing 55.8
g of MgCl2 dissolved in 1.00 L of solution?

A sulfuric acid solution containing 571.5 g of H2 SO4 per liter of aqueous solution has a density of 1.329 g/cm3.Calculate the molarity of H2 SO4 in this solution.

Ascorbic acid (vitamin C, C6H8O6) is a water-soluble vitamin. A solution containing 81.5 g of ascorbic acid dissolved in 220 g of water has a density of 1.22 g/mL at 55oC.
You may want to reference (Pages 538 - 541)Section 13.4 while completing this problem.Calculate the molarity of ascorbic acid in this solution.

What is the molarity of each of the following solutions?15.5 g
Al2 (SO4 )3 in 0.250 L solution

What is the molarity of each of the following solutions?5.25 g
Mn(NO3 )2 2H2 O in 175 mL of solution

A strontium hydroxide solution is prepared by dissolving 10.45 g of Sr(OH)2 in water to make 53.00 mL of solution.What is the molarity of this solution?

What is molarity?

You may want to reference (Pages 144 - 148)Section 4.5 while completing this problem.What is the molarity of a solution that is made by dissolving 3.68 g of sucrose (C12H22O11) in sufficient water to form 275.0 mL of solution?

The concentration of alcohol (CH3CH2OH) in blood, called the "blood alcohol concentration" or BAC, is given in units of grams of alcohol per 100 mL of blood. The legal definition of intoxication in many states of the United States is a BAC of 0.08 or higher.
You may want to reference (Pages 145 - 148) Section 4.5 while completing this problem.What is the concentration of alcohol, in terms of molarity, in blood if the BAC is 0.08?

Which will have the highest concentration of potassium ion: 0.20 M
KCl, 0.15 M
K2CrO4, or 0.080 M
K3PO4?

Indicate the concentration of each ion or molecule present in the following solutions.0.35
M
NaNO3

Indicate the concentration of each ion or molecule present in the following solutions.2.3×10−2
M
MgSO4

You may want to reference (Pages 144 - 148)Section 4.5 while completing this problem.What is the ratio of the concentration of potassium ions to the concentration of carbonate ions in a 0.015 M solution of potassium carbonate?

Indicate the concentration of each ion or molecule present in the following solutions.3.00×10−2
M
C6H12O6

Indicate the concentration of each ion or molecule present in the following solutions.A mixture of 45.0mL of 0.272M
NaCl and 65.0mL of 0.0247M
(NH4)2CO3. Assume that the volumes are additive.

You may want to reference (Pages 145 - 148) Section 4.5 while completing this problem.
Indicate the concentration of each ion present in the solution formed by mixing the following.42.0 mL of 0.170
M
NaOH and 37.6 mL of 0.410
M
NaOH. Assume that the volumes are additive.

You may want to reference (Pages 145 - 148) Section 4.5 while completing this problem.
Indicate the concentration of each ion present in the solution formed by mixing the following.44.0 mL of 0.130
M
Na2SO4 and 25.0 mL of 0.180
M
KCl. Assume that the volumes are additive.

You may want to reference (Pages 145 - 148) Section 4.5 while completing this problem.
Indicate the concentration of each ion present in the solution formed by mixing the following.3.60 g
KCl in 75.0 mL of 0.260
M
CaCl2 solution. Assume that the volumes are additive.

You may want to reference (Pages 152 - 157) Section 4.4 while completing this problem.Calculate the molarity of a solution made by adding 45.1 g of NaNO3 to a flask and dissolving with water to a total volume of 2.50 L .

An aqueous solution contains 2.4 mM of total ions.If the solution is NaCl (aq), what is the concentration of chloride ion?

An aqueous solution contains 2.4 mM of total ions.If the solution is FeCl3 (aq), what is the concentration of chloride ion?

Calculate the molarity of a solution that contains 0.180 mol
ZnCl2 in exactly 160 mL of solution.

You may want to reference(Pages 144 - 148)Section 4.5 while completing this problem.Calculate the molarity of a solution prepared by dissolving 12.5 g of Na2CrO4 in enough water to produce a solution with a volume of 750. mL .

Calculate the molarity of each of the following solutions.4.25 mol of LiCl in 2.90 L solution

Calculate the molarity of each of the following solutions.28.03 g
C6 H12 O6 in 1.24 L of solution

Calculate the molarity of each of the following solutions.35.6 mg
NaCl in 119.5 mL of solution

What is the molarity of NO3- in each solution?0.160 M
KNO3.

What is the molarity of NO3- in each solution?0.260 M Ca(NO3)2.

What is the molarity of NO3- in each solution?0.360 M
Al(NO3)3.

What is the molarity of Cl- in each solution?
You may want to reference (Pages 152 - 157) Section 4.4 while completing this problem.0.210 M
NaCl

What is the molarity of Cl- in each solution?
You may want to reference (Pages 152 - 157) Section 4.4 while completing this problem.0.160 M
SrCl2

What is the molarity of Cl- in each solution?
You may want to reference (Pages 152 - 157) Section 4.4 while completing this problem.0.110M
AlCl3

You may want to reference (Pages 152 - 157) section 4.4 while completing this problem.
Calculate the molarity of each of the following solutions.0.41 mol of LiNO3 in 6.26 L of solution

You may want to reference (Pages 152 - 157) section 4.4 while completing this problem.
Calculate the molarity of each of the following solutions.12.21 mg
KI in 107.6 mL of solution

Ammonium chloride, NH4Cl, is a very soluble salt in water.If you dissolve 16 g of ammonium chloride in 500.0 mL
of water, what is the molar concentration of the solution?

What is the total concentration of ions in a 1.1 M solution of ammonium sulfate?
A. 1.1 M
B. 2.2 M
C. 3.3 M
D. 4.4 M
E. 18.7 M

What is the concentration of nitrate ions in a 0.125 M Mg(NO 3)2 solution?
A) 0.375 M
B) 0.0625 M
C) 0.125 M
D) 0.160 M
E) 0.250 M

Calculate the molarity of a saturated solution of sodium hydrogen carbonate (baking soda), NaHCO3(aq) that contains 69.0 grams in 1.00 liter of solution.

What is the concentration of K+ ions in a 0.045 M K 2CO3 solution assuming complete dissociation?

You have a solution of table salt in water. What happens to the salt concentration (increases, decreases, or stays the same) as the solution boils? Draw pictures to explain your answer.

a. At 30°C , the molar solubility of barium sulfate in water is 1.2 x 10 -5 M . Calculate the solubility in grams per liter.b. How many liters of water are required to dissolve 1 g of barium sulfate?

A solution of ammonia is made by dissolving 35 g NH 3 in 90.0 g of H2O. The density of the solution is 0.898 g/mL. What is the molarity of NH3?d = Mass / Volumea) 53 Mb) 0.39 Mc) 23 Md) 15 Me) not possible to calculate

The molecular weight of ethanol (C2H5OH) is 46.1 and the density of absolute (100%) ethanol = 0.79 g/mL
a) Calculate the molarity of absolute ethanol (100% ethanol).
b) Calculate the molarity of ethanol in a bottle of wine that is 14.0% ethanol by volume.

The molecular weight of ethanol (C2H5OH) is 46.1 and the density of absolute (100%) ethanol = 0.79 g/mL
The legal limit for a driver’s blood alcohol is 50 mg of ethanol per 100 mL of blood (referred to as a blood alcohol content (BAC) of 0.05%). What is the molarity of ethanol (in blood) in a person at this legal limit?

(a) Is the concentration of a solution an intensive or an extensive property?

(b) What is the difference between 0.50 mol HCl and 0.50 M HCl?

(a) Suppose you prepare 500 mL of a 0.10 M solution of some salt and then spill some of it. What happens to the concentration of the solution left in the container?

What number of grams of KBr are needed to prepare 50.0 mL a 0.716 M solution?A. 4.26 gB. 3.58 gC. 0.0358 gD. 4,260 gE. 0.00358 g

(b) Suppose you prepare 500 mL of a 0.10 M aqueous solution of some salt and let it sit out, uncovered, for a long time, and some water evaporates. What happens to the concentration of the solution left in the container?

What is the molarity of a solution that contains 17g of NH 3 in 0.50 L of solution.

(c) A certain volume of a 0.50 M solution contains 4.5 g of a salt. What mass of the salt is present in the same volume of a 2.50 M solution?

A scientist wants to make a solution of tribasic sodium phosphate, Na 3PO4, for a laboratory experiment. How many grams of Na 3PO4 will be needed to produce 575 mL of a solution that has a concentration of Na+ ions of 0.600 M ?

Spongebob Squarepants dissolved 4.96 g HNO3 in enough water to make 269 mL of solution.What was the molarity of his solution?a) 3.41b) 0.293c) 0.0242d) 18.43e) 0.0184

Oxalic acid dihydrate, H2C2O4 * 2 H2O (molar mass = 126.07 g/mol) is often used as a primary standard for the standardization of an NaOH solution. If 0.147 g of oxalic acid dihydrate are neutralized by 23.64 mL of an NaOH solution, what is the molar concentration of the NaOH solution? Oxalic acid is a diprotic acid. (What is the balanced equation?)

(a) Calculate the molarity of a solution made by dissolving 0.750 grams of Na 2SO4 in enough water to form exactly 850 mL of solution.

(b) How many moles of KMnO4 are present in 250 mL of a 0.0475 M solution?

Calculate the molarity of each of the following solutions.a. 0.41 mol of LiNO3 in 6.26 L of solutionb. 72.9 g C2H6O in 2.35 L of solutionc. 12.21 mg KI in 107.6 mL of solution

(c) How many milliliters of 11.6 M HCl solution are needed to obtain 0.250 mol of HCl?

The average adult human male has a total blood volume of 5.0 L. If the concentration of sodium ion in this average individual is 0.135 M, what is the mass of sodium ion circulating in the blood?

A person suffering from hyponatremia has a sodium ion concentration in the blood of 0.118 M and a total blood volume of 4.6 L. What mass of sodium chloride would need to be added to the blood to bring the sodium ion concentration up to 0.138 M, assuming no change in blood volume?

Which of the solutions below have the same molar concentration as Solution X?

(a) How many grams of solute are present in 50.0 mL of 0.488 M K 2Cr2O7?

(b) If 4.00 g of (NH 4)2SO4 is dissolved in enough water to form 400 mL of solution, what is the molarity of the solution?

How many moles of NaCl are required to make 250 mL of a 3.00 M solution?a. 750 molesb. 0.750 molesc. 0.250 molesd. 3 moles

(c) How many milliliters of 0.0250 M CuSO4 contain 1.75 g of solute?

If you want to double the concentration of a solution, how could you do it?

In each of the following pairs, indicate which has the higher concentration of Cl – ion: (a) 0.10 M CaCl2 or 0.15 M KCI solution

In each of the following pairs, indicate which has the higher concentration of Cl– ion: (b) 100 mL of 0.10 M KCI solution or 400 mL of 0.080 M LiCI solution

An average human being has about 5.0 L of blood in his or her body. If an average person were to eat 32.0 g of sugar (sucrose, C12H22O11, 342.30 g/mol), and all that sugar were dissolved into the bloodstream, how would the molarity of the blood sugar change?

In each of the following pairs, indicate which has the higher concentration of Cl – ion: (c) 0.050 M HCl solution or 0.020 M CdCl2 solution.

What volume of a 0.716 M KBr solution is needed to provide 30.5 g of KBr?A. 21.8 mLB. 42.7 mLC. 184 mLD. 357 mL

Indicate the concentration of each ion or molecule present in the following solutions: (a) 0.25 M NaNO3Assume that the volumes are additive.

Indicate the concentration of each ion or molecule present in the following solutions: (b) 1.3 x 10–2 MgSO4Assume that the volumes are additive.

Indicate the concentration of each ion or molecule present in the following solutions: (d) a mixture of 45.0 mL of 0.272 M NaCl and 65.0 mL of 0.0247 M (NH4)2CO3. Assume that the volumes are additive.

Acetylsalicylic acid is the active ingredient in aspirin. It took 35.17 mL of 0.5065 M sodium hydroxide to react completely with 3.210 g of acetylsalicylic acid. Acetylsalicylic acid has one acidic hydrogen. What is the molar mass of acetylsalicylic acid?

Indicate the concentration of each ion present in the solution formed by mixing (a) 42.0 mL of 0.170 M NaOH and 37.6 mL of 0.400 M NaOH. Assume that the volumes are additive.

Determine the molarity of a solution formed by dissolving 468 mg of MgI 2 in enough water to yield 50.0 mL of solution. A) 0.0297 MB) 0.0337 MC) 0.0936 MD) 0.0107 ME) 0.0651 M

Indicate the concentration of each ion present in the solution formed by mixing (b) 44.0 mL of 0.100 M and Na2SO4 and 25.0 mL of 0.150 M KCl. Assume that the volumes are additive.

Indicate the concentration of each ion present in the solution formed by mixing (c) 3.60 g KCl in 75.0 mL of 0.250 M CaCl2 solution. Assume that the volumes are additive.

What does this statement mean? 2.35 M LiF

What is the concentration of nitrate ions in a solution that contains 74.5 g lead (IV) nitrate, Pb(NO3)4, dissolved in 450 mL solution? ( MW of Pb(NO3)4 is 455.24 g/mol).

Pure acetic acid, known as glacial acetic acid, is a liquid with a density of 1.049 g/mL at 25°C. Calculate the molarity of a solution of acetic acid made by dissolving 20.00 mL of glacial acetic acid at 25°C in enough water to make 250.0 mL of solution.

Glycerol, C3H8O3, is a substance used extensively in the manufacture of cosmetics, foodstuffs, antifreeze, and plastics. Glycerol is a water-soluble liquid with a density of 1.2656 g/L at 15°C. Calculate the molarity of a solution of glycerol made by dissolving 50.000 mL glycerol at 15°C in enough water to make 250.00 mL of solution.

When hydrochloric acid reacts with magnesium metal, hydrogen gas and aqueous magnesium chloride are produced. What volume of 5.0 M HCl is required to react completely with 3.00 g of magnesium?

Douglasite is a mineral with the formula 2KCl • FeCl 2 • 2H2O. Calculate the mass percent of douglasite in a 455.0-mg sample if it took 37.20 mL of a 0.1000 M AgNO3 solution to precipitate all the Cl– as AgCl. Assume the douglasite is the only source of chloride ion.

The concentration of distilled white vinegar is written as 5% (w/v) of acetic acid (CH3COOH). Convert the concentration in the unit of molarity. Express your answer in four significant figures.

Calculate the concentration of all ions present when 0.160 g of MgCl 2 is dissolved in 100.0 mL of solution.

Determine the mass (g) of solute required to form 275 mL of a 0.4230 M KClO 3 solution.a. 1.97b. 4.21c. 14.3d. 12.2e. 19.6

What mass of FeCl2 is needed to prepare 750.0 mL of 2.00 M solution?(A) 47.6 g(B) 95.3 g(C) 127 g(D) 190.5 g(E) 190,500 g

What is the molarity of Cl− in each solution?
A) 0.170 M NaCl.
B) 0.150 M SrCl2.

1) What is the concentration of K + in 0.15 M of K 2S?
2) If CaCl2 is dissolved in water, what can be said about the concentration of the Ca 2+ ion?
a. It has the same concentration as the Cl − ion.
b. Its concentration is half that of the Cl − ion.
c. Its concentration is twice that of the Cl − ion.
d. Its concentration is one-third that of the Cl − ion.

Calculate the molarity of each of these solutions.a. A 5.623-g sample of NaHCO3 is dissolved in enough water to make 250.0 mL of solution.

Calculate the molarity of each of these solutions. b. A 184.6-mg sample of K 2Cr2O7 is dissolved in enough water to make 500.0 mL of solution.

A chemist wants to make 5.0 L of a 0.260 M CaCl2 solution. What mass of CaCl2 (in g) should the chemist use?

A solution of ethanol (C2H5OH) in water is prepared by dissolving 75.0 mL of ethanol (density = 0.79 g/cm3) in enough water to make 250.0 mL of solution. What is the molarity of the ethanol in this solution?

What is the concentration of nitrate ions in a 0.125 M Mg(NO 3)2 solution?a. 0.0625 Mb. 0.160 Mc. 0.250 Md. 0.125 Me. 0.375 M

Calculate the concentration of all ions present in each of the following solutions of strong electrolytes.a. 0.100 mol of Ca(NO3)2 in 100.0 mL of solution

Calculate the concentration of all ions present in each of the following solutions of strong electrolytes.b. 2.5 mol of Na 2SO4 in 1.25 L of solution

A person suffering from hyponatremia has a sodium ion concentration of 0.118 M in his blood and has a total blood volume of 4.6 L. What mass of sodium chloride would need to be added to the blood to bring the sodium ion concentration to 0.138 M with no change in blood volume?

Calculate the concentration of all ions present in each of the following solutions of strong electrolytes.c. 5.00 g of NH 4Cl in 500.0 mL of solution

Which of the following solutions has the largest concentration of solvated protons: (a) 0.2 M LiOH, (b) 0.2 M HI, (c) 1.0 M methyl alcohol (CH3OH)? Explain

Which of the following solutions is the most basic? (a) 0.6 M NH 3, (b) 0.150 M KOH, (c) 0.100 M Ba(OH)2. Explain.

Calculate the concentration of all ions present in each of the following solutions of strong electrolytes.d. 1.00 g K3PO4 in 250.0 mL of solution

Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molarity of the HCl, if the solution has a density of 1.20 g/mL.
A) 13.9 M
B) 12.8 M
C) 10.7 M
D) 9.35 M
E) 7.79 M

Calculate the concentration of all ions present in each of the following solutions of strong electrolytes.a. 0.0200 mol of sodium phosphate in 10.0 mL of solution

Calculate the concentration of all ions present in each of the following solutions of strong electrolytes.b. 0.300 mol of barium nitrate in 600.0 mL of solution

Calculate the concentration of all ions present in each of the following solutions of strong electrolytes.c. 1.00 g of potassium chloride in 0.500 L of solution

Calculate the concentration of all ions present in each of the following solutions of strong electrolytes.d. 132 g of ammonium sulfate in 1.50 L of solution

Which of the following solutions of strong electrolytes contains the largest number of moles of chloride ions: 100.0 mL of 0.30 M AlCl3, 50.0 mL of 0.60 M MgCl 2, or 200.0 mL of 0.40 M NaCl?

A student titrates an unknown amount of potassium hydrogen phthalate (KHC 8H4O4, often abbreviated KHP) with 20.46 mL of a 0.1000 M NaOH solution. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. What mass of KHP was titrated (reacted completely) by the sodium hydroxide solution?

What mass of NaOH is contained in 250.0 mL of a 0.400 M sodium hydroxide solution?

A solution was prepared by dissolving 39.0 g of KCl in 225 mL of water. Calculate the molarity of KCl in the solution if the total volume of the solution is 239 mL.

If 10. g of AgNO3 is available, what volume of 0.25 M AgNO3 solution can be prepared?

Calculate the molarity of each of the following solutions.a. 0.50mol of LiNO3 in 6.50L of solutionb. 72.2g C2H6O in 2.43L of solutionc. 12.72 mg KI in 113.6 mL of solution

How many milligrams of NaCN are required to prepare 712 mL of 0.250 M NaCN?

How many moles of sodium ions are in 35.0 ml of a 0.750 M NaCl(aq) solution?
A. 0.0263 moles
B. 0.750 moles
C. 0.0523 moles
D. 0.375 moles
E. 0.131 moles

Calculate the sodium ion concentration when 70.0 mL of 3.0 M sodium carbonate is added to 30.0 mL of 1.0 M sodium bicarbonate.

What volume, in liters, of a 2.00 M KCl solution contains 2.5 g of KCl? (Molar mass KCl = 74.55 g/mole)

38. A solution was prepared by mixing 50.00 mL of 0.100 M HNO 3 and 100.00 mL of 0.200 M HNO3. Calculate the molarity of the final solution of nitric acid.

Calculate the molarity of the following solutions. a. 0.600 mol of Na 2S in 1.40 L of solution.b. 20.1 g of MgS in 851 mL of solution.

How many liters of a 0.0550 M KCl solution contain 0.163 moles of KCl?
A) 1.12 L
B) 3.37 L
C) 8.97 L
D) 2.96 L
E) 1.48 L

How many moles of LiI are contained in 258.6 mL of 0.0296 M LiI solution?A) 8.74 × 10-3 molB) 1.31 × 10-3 molC) 1.14 × 10-3 molD) 3.67 × 10-3 molE) 7.65 × 10-3 mol

What mass of copper (II) acetate (Cu(C2H3O2)2 141.64 g/mol) is required to produce 500.0 mL of a 1.27M solution of copper(II) acetate?

Calculate each of the following quantities:Volume (mL) of 6.44×10−2 M adenosine triphosphate (ATP) that contains 1.68 mmol of ATP

Calculate each of the following quantities:Volume (L) of 0.385 M manganese(II) sulfate that contains 63.0 g of solute

What volume of a 0.20-M K2SO4 solution contains 57 g of K2SO4?

If 10. g of AgNO3 is available, what volume of 0.25 M AgNO3 solution can be prepared?

Calculate each of the following quantities:Volume (mL) of 2.26 M potassium hydroxide that contains 8.42 g of solute

Calculate each of the following quantities:Number of Mg2+ ions in each milliliter of 0.184 M magnesium bromide

How many moles of solute particles are present in 1 L of each of the following aqueous solutions? (a) 0.3 M KBr

How many moles of solute particles are present in 1 L of each of the following aqueous solutions?(b) 0.065 M HNO3

How many moles of solute particles are present in 1 L of each of the following aqueous solutions?(c) 10–4 M KHSO4

How many moles of solute particles are present in 1 L of each of the following aqueous solutions?(d) 0.06 M ethanol (C2H5OH)

How many moles and how many ions of each type are present in each of the following?130 mL of 0.45 M aluminum chloride

How many moles and how many ions of each type are present in each of the following?9.80 mL of a solution containing 2.59 g lithium sulfate/L

How many moles and how many ions of each type are present in each of the following?245 mL of a solution containing 3.68×1022 formula units of potassium bromide per liter

How many moles of solute particles are present in 1 mL of each of the following aqueous solutions?(a) 0.02 M CuSO4

How many moles of solute particles are present in 1 mL of each of the following aqueous solutions?(b) 0.004 M Ba(OH)2

How many moles and how many ions of each type are present in each of the following?88 mL of 1.75 M magnesium chloride

How many moles of solute particles are present in 1 mL of each of the following aqueous solutions? (c) 0.08 M pyridine (C5H5N)

How many moles and how many ions of each type are present in each of the following?321 mL of a solution containing 0.22 g aluminum sulfate/L

How many moles of solute particles are present in 1 mL of each of the following aqueous solutions?(d) 0.05 M (NH4)2CO3

How many moles and how many ions of each type are present in each of the following?1.65 L of a solution containing 8.83×1021 formula units of cesium nitrate per liter

Consider this question: What is the mass of the solute in 0.500 L of 0.30 M glucose, C6H12O6, used for intravenous injection? (a) Outline the steps necessary to answer the question. (b) Answer the question.

Consider this question: What is the mass of solute in 200.0 L of a 1.556-M solution of KBr? (a) Outline the steps necessary to answer the question. (b) Answer the question.

Calculate the number of moles and the mass of the solute in each of the following solutions: (a) 2.00 L of 18.5 M H2SO4, concentrated sulfuric acid

You wish to prepare 1 L of a 0.02-M potassium iodate solution. You require that the final concentration be within 1% of 0.02 M and that the concentration must be known accurately to the fourth decimal place. How would you prepare this solution? Specify the glassware you would use, the accuracy needed for the balance, and the ranges of acceptable masses of KIO3 that can be used.

Calculate the number of moles and the mass of the solute in each of the following solutions:(b) 100.0 mL of 3.8 × 10−5 M NaCN, the minimum lethal concentration of sodium cyanide in blood serum

Calculate the number of moles and the mass of the solute in each of the following solutions:(c) 5.50 L of 13.3 M H2CO, the formaldehyde used to “fix” tissue samples

Calculate the number of moles and the mass of the solute in each of the following solutions:(d) 325 mL of 1.8 × 10−6 M FeSO4, the minimum concentration of iron sulfate detectable by taste in drinking water

Calculate the number of moles and the mass of the solute in each of the following solutions: (a) 325 mL of 8.23 × 10−5 M KI, a source of iodine in the diet

Calculate the number of moles and the mass of the solute in each of the following solutions:(b) 75.0 mL of 2.2 × 10−5 M H2SO4, a sample of acid rain

Calculate the number of moles and the mass of the solute in each of the following solutions:(c) 0.2500 L of 0.1135 M K2CrO4, an analytical reagent used in iron assays

Calculate the number of moles and the mass of the solute in each of the following solutions:(d) 10.5 L of 3.716 M (NH4)2SO4, a liquid fertilizer

How many moles of H+ ions are present in each of the following aqueous solutions?1.40 L of 0.25 M perchloric acid

How many moles of H+ ions are present in each of the following aqueous solutions?6.8 mL of 0.92 M nitric acid

How many moles of H+ ions are present in each of the following aqueous solutions?2.6 L of 0.085 M hydrochloric acid

What mass of NaOH is contained in 250.0 mL of a 0.400 M sodium hydroxide solution?

Describe how you would prepare 2.00 L of 0.250 M NaOH from solid NaOH.

Describe how you would prepare 2.00 L of 0.100 M K2CrO4 from solid K2CrO4.

How would you prepare 1.00 L of a 0.50-M solution of NiCl 2 from the salt NiCl 2 • 6 H2O?

How would you prepare 1.00 L of a 0.50-M solution of s odium carbonate from the pure solid?

How many moles of H+ ions are present in each of the following aqueous solutions?1.4 mL of 0.75 M hydrobromic acid

How many moles of H+ ions are present in each of the following aqueous solutions?2.47 mL of 1.98 M hydriodic acid

How many moles of H+ ions are present in each of the following aqueous solutions?395 mL of 0.270 M nitric acid

How many total moles of ions are released when each of the following dissolves in water?0.32 mol of NH4Cl

How many total moles of ions are released when each of the following dissolves in water?0.805 mol of Rb2SO4

How many total moles of ions are released when each of the following dissolves in water?0.75 mol of K3PO4

How many total moles of ions are released when each of the following dissolves in water?25.4 g of Ba(OH)2·8H2O

How many total moles of ions are released when each of the following dissolves in water?3.55×1019 formula units of LiCl

How many total moles of ions are released when each of the following dissolves in water?3.85×10−3 g of Ca(NO3)2

How many total moles of ions are released when each of the following dissolves in water?4.03×1019 formula units of Sr(HCO3)2

How many total moles of ions are released when each of the following dissolves in water?6.88×10−3 g of NiBr2·3H2O

How many total moles of ions are released when each of the following dissolves in water?2.23×1022 formula units of FeCl3

How many total moles of ions are released when each of the following dissolves in water?0.734 mol of Na2HPO4

How many total moles of ions are released when each of the following dissolves in water?3.86 g of CuSO4·5H2O

How many total moles of ions are released when each of the following dissolves in water?8.66×1020 formula units of NiCl2

Calculate each of the following quantities:Mass (g) of solute in 185.8 mL of 0.267 M calcium acetate

Calculate each of the following quantities:Amount (mol) of solute in 145.6 L of 0.850 M sodium cyanide

Calculate each of the following quantities:Number of Cu2+ ions in 52 L of 2.3 M copper(II) chloride

Calculate each of the following quantities:Mass (g) of solute needed to make 475 mL of 5.62×10−2 M potassium sulfate

The concentration of alcohol CH3CH2OH in blood, called the blood alcohol concentration or BAC, is given in units of grams of alcohol per 100mL of blood.What is the concentration of the alcohol, in terms of molarity in blood if the BAC is 0.08?

Calculate each of the following quantities:Molarity of a solution that contains 7.25 mg of calcium chloride in each milliliter

Calculate each of the following quantities:Molarity of the solution resulting from dissolving 46.0 g of silver nitrate in enough water to give a final volume of 335 mL

You are given solutions of HCl and NaOH and must determine their concentrations. You use 27.5 mL of NaOH to titrate 100. mL of HCl and 18.4 mL of NaOH to titrate 50.0 mL of 0.0782 M H2SO4. Find the unknown concentrations.

The flask represents the products of the titration of 25 mL of sulfuric acid with 25 mL of sodium hydroxide.What are the molarities of the acid and the base?

When 13.63
g (about one tablespoon) of table sugar (sucrose,
C12H22O11) is dissolved in 241.5 mL of water (density 0.997 g/mL), the final volume is 250.0 mL (about one cup). What is the molarity of the table sugar?

What information do we need to calculate the molarity of a sulfuric acid solution?

What does it mean when we say that a 200-mL sample and a 400-mL sample of a solution of salt have the same molarity? In what ways are the two samples identical? In what ways are these two samples different?

Determine the molarity for each of the following solutions:(a) 0.444 mol of CoCl2 in 0.654 L of solution

Determine the molarity for each of the following solutions:(c) 0.2074 g of calcium hydroxide, Ca(OH)2, in 40.00 mL of solution

Determine the molarity for each of the following solutions:(d) 10.5 kg of Na2SO4∙10H2O in 18.60 L of solution

Determine the molarity for each of the following solutions:(e) 7.0 × 10−3 mol of I2 in 100.0 mL of solution

Determine the molarity for each of the following solutions:(f) 1.8 × 104 mg of HCl in 0.075 L of solution

Determine the molarity for each of the following solutions:(b) 98.0 g of phosphoric acid, H3PO4, in 1.00 L of solution

Determine the molarity of each of the following solutions:(a) 1.457 mol KCl in 1.500 L of solution

Determine the molarity of each of the following solutions:(b) 0.515 g of H2SO4 in 1.00 L of solution

Determine the molarity of each of the following solutions:(c) 20.54 g of Al(NO3)3 in 1575 mL of solution

Determine the molarity of each of the following solutions:(d) 2.76 kg of CuSO4∙5H2O in 1.45 L of solution

Determine the molarity of each of the following solutions:(e) 0.005653 mol of Br2 in 10.00 mL of solution

Ordinary household bleach is an aqueous solution of sodium hypochlorite. What is the molarity of a bleach solution that contains 20.5 g of sodium hypochlorite in 375 mL? 20.5 g of sodium hypochlorite in 375 mL?

Determine the molarity of each of the following solutions:(f) 0.000889 g of glycine, C2H5NO2, in 1.05 mL of solution

A solution is prepared by dissolving 28.6 g of glucose (C6H12O6) in 360 g of water. The final volume of the solution is 380 mL. For this solution, calculate each of the following.Molarity

Consider this question: What is the molarity of KMnO4 in a solution of 0.0908 g of KMnO4 in 0.500 L of solution? (a) Outline the steps necessary to answer the question. (b) Answer the question.

An average human being has about 5.0 L of blood in his or her body. If an average person were to eat 32.0 g of sugar (sucrose, C12H22O11, 342.30 g/mol), and all that sugar were dissolved into the bloodstream, how would the molarity of the blood sugar change?

Consider this question: What is the molarity of HCl if 35.23 mL of a solution of HCl contain 0.3366 g of HCl? (a) Outline the steps necessary to answer the question. (b) Answer the question.

Calculate the molarity of each of the following solutions:(a) 0.195 g of cholesterol, C27H46O, in 0.100 L of serum, the average concentration of cholesterol in human serum

You may want to reference (Page) Section 13.5 while completing this problem.A solution is prepared by dissolving 20.2 mL of methanol (CH3OH) in 100.0 mL of water at 25 oC. The final volume of the solution is 118 mL. The densities of methanol and water at this temperature are 0.782 g/mL and 1.00 g/mL, respectively. For this solution, calculate each of the following.Molarity

Calculate the molarity of each of the following solutions:(b) 4.25 g of NH3 in 0.500 L of solution, the concentration of NH3 in household ammonia

Calculate the molarity of each of the following solutions:(c) 1.49 kg of isopropyl alcohol, C3H7OH, in 2.50 L of solution, the concentration of isopropyl alcohol in rubbing alcohol

Calculate the molarity of each of the following solutions:(d) 0.029 g of I2 in 0.100 L of solution, the solubility of I2 in water at 20 °C

Calculate the molarity of each of the following solutions: (a) 293 g HCl in 666 mL of solution, a concentrated HCl solution

Calculate the molarity of each of the following solutions:(b) 2.026 g FeCl3 in 0.1250 L of a solution used as an unknown in general chemistry laboratories

Calculate the molarity of each of the following solutions:(c) 0.001 mg Cd2+ in 0.100 L, the maximum permissible concentration of cadmium in drinking water

Two 25.0-mL aqueous solutions, labeled A and B, contain the ions indicated:What is the molarity of B?

Calculate the molarity of each of the following solutions:(d) 0.0079 g C7H5SNO3 in one ounce (29.6 mL), the concentration of saccharin in a diet soft drink.

There is about 1.0 g of calcium, as Ca2+, in 1.0 L of milk. What is the molarity of Ca2+ in milk?

A 2.00-L bottle of a solution of concentrated HCl was purchased for the general chemistry laboratory. The solution contained 868.8 g of HCl. What is the molarity of the solution?

Calculate the molarity of each aqueous solution:(a) 32.3 g of table sugar (C12H22O11) in 100. mL of solution

Calculate the molarity of each aqueous solution:(b) 5.80 g of LiNO3 in 505 mL of solution

Calculate the molarity of each aqueous solution: (a) 0.82 g of ethanol (C2H5OH) in 10.5 mL of solution

Calculate the molarity of each aqueous solution:(b) 1.27 g of gaseous NH3 in 33.5 mL of solution

Calculate the molarity of a 5.623-g sample of NaHCO 3 is dissolved in enough water to make 250.0 mL of solution.

Calculate the molarity of a 184.6-mg sample of K 2Cr2O7 is dissolved in enough water to make 500.0 mL of solution.

Calculate the molarity of a 0.1025-g sample of copper metal is dissolved in 35 mL of concentrated HNO3 to form Cu2+ ions and then water is added to make a total volume of 200.0 mL. (Calculate the molarity of Cu2+.)

A solution of ethanol (C2H5OH) in water is prepared by dissolving 75.0 mL of ethanol (density = 0.79 g/cm3) in enough water to make 250.0 mL of solution. What is the molarity of the ethanol in this solution?

You may want to reference (Pages 586 - 592) Section 13.5 while completing this problem.An aqueous KNO3 solution is made using 77.6 g of KNO3 diluted to a total solution volume of 1.96 L. (Assume a density of 1.05 g/mL for the solution)Calculate the molarity of the solution.

Write a detailed set of instructions for making two solutions: (1) 100 mL of 16 MNaOH from solid sodium hydroxide and (2) 1.00 L of 0.1 M NaOH from your first solution. You have in your lab: volumetric flasks marked to contain 100.0 mL and 1.000 L,
a graduated cylinder, and a balance.Write a detailed set of instruction for making a 100 mL solution of 16 M NaOH.

You may want to reference (Pages 152 - 157) section 4.4 while completing this problem.Calculate the molarity of each of the following solutions.72.9 g C2H6O in 2.35 L of solution

Write a detailed set of instructions for making two solutions: (1) 100 mL of 16 MNaOH from solid sodium hydroxide and (2) 1.00 L of 0.1 M NaOH from your first solution. You have in your lab: volumetric flasks marked to contain 100.0 mL and 1.000 L,
a graduated cylinder, and a balance.Write a detailed set of instruction for making a 1.00 L solution of 0.1 M NaOH.

Calculate each of the following quantities:Molarity of 500. mL of solution containing 21.1 g of potassium iodide

You may want to reference (Pages 586 - 592) Section 13.5 while completing this problem.A solution is prepared by dissolving 50.5 g sucrose (C12H22O11) in 0.404 kg of water. The final volume of the solution is 355 mL. For this solution, calculate molarity.

Calculate each of the following quantities:Molarity of 275 mL of solution containing 135 mmol of glucose

Enter your answer in the provided box. What volume (in milliliters of a 0.795 M NaOH solution contains 3.45 g of NaOH?

How many moles of MgCl2 are present in 47.5 mL of 0.160 M MgCl2 solution?

What is the molarity of ZnCl2 that forms when 30.0 g of zinc completely reacts with CuCl2 according to the following reaction? Assume a final volume of 285 mL.Zn(s) + CuCl2 (aq) ---> ZnCl2(aq) + Cu(s)

Calculate the volume of a 0.921 M sulfuric acid (H2SO4) solution containing 0.236 mol of solute. Enter your answer in the provided box.

What volume of a 0.39 M Mg(NO3)2 solution contains 92 g of Mg(NO3)2? Express your answer using two significant figures.

How many moles of solute are present in the following solutions?Part A 135 mL of 0.33 M NaNO3Part B 370 mL of 1.4 M HNO3

Calculate the volume in millimeters of a 3.4M calcium bromide solution that contains 200 g of calcium bromide (CaBr2). Be sure your answer has the correct number of significant digits.

When solutions of silver nitrate and potassium chloride are mixed, silver chloride precipitates out of solution according to the equationAgNO3(aq) + KCl(aq) --> AgCl(s) + KNO3(aq)What mass of silver chloride can be produced from 1.97 L of a 0.232 M solution of silver nitrate? Express your answer with the appropriate units.The reaction described in Part A required 3.65 L of potassium chloride. What is the concentration of this potassium chloride solution? Express your answer with the appropriate units.

What volume (in milliliters) of a 0.615 M NaOH solution contains 9.35 g of NaOH? Enter your answer in scientific notation.

Calculate the mass of KI in grams required to prepare 5.00x102 mL of a 1.5 M solution

Enter your answer in the provided box.An aqueous solution that is 50.0 percent sulfuric acid (H2SO4) by mass has a density of 1.146 g/mL. Determine the molarity of the solution.

Calculate the molarity of 0.750 mol of Na2S in 1.60 L of solution. Caloulate the molarity of 31.7 g of MgS in 845 mL of solution.

Calculate the volume in liters of a 3.3 x 10 -4 μM magnesium fluoride solution that contains 400 mmol of magnesium fluoride (MgF2). Round your answer to 2 significant digits.

A laboratory procedure calls for making 450.0 mL of a 1.2 M NaNO3 solution. What mass of NaNO3 (in g) is needed?

The end point of a titration was reached after 28 mL of 0.05 M disodium EDTA titrant was dispensed into a solution containing the zinc ion. Calculate the moles of disodium EDTA used.

What is the molar concentration of Na + ions in 0.025 M solutions of the following sodium salts in water?

How many grams of NaOH (MW = 40.0) are there in 350.0 mL of a 0.225 M NaOH solution?

Calculate the molarity of the two solutions. a) 0.300 mol of NaOH in 1.80 L of solution. b) 14.7 g of NaCI in 719 mL of solution.

If 7.01 g of CuNO3 is dissolved in water to make a 0.510 M solution, what is the volume of the solution?

How many mL of a 0.181 M aqueous solution of cobalt(II) fluoride, CoF 2, must be taken to obtain 7.40 grams of the salt?_____mL

Calculate the molarity of the two solutions.a. 0.400 mol of NaOH in 2.75 L of solution.b. 11.5 g of NaCl in 707 mL of solution.

How many liters of a 0.0550 M LiF solution contain 0.163 moles of LiF?a. 8.97 Lb. 1.48 Lc. 3.37 Ld. 1.12 Le. 2.96 L

Concentrated aqueous hydrochloric acid is 37.2 wt% HCl and has a concentration of 12.1 M. Calculate the volume of concentrated hydrochloric acid that should be diluted to 1.40 L to form a 4.10 MHCl solution. Determine the density of 37.2 wt% HCl.

Calculate the molarity of the two solutions.a. 0.150 mol of NaOH in 1.70 L of solution. b. 16.9 g of NaCl in 687 mL of solution.

How many moles of nitrate ion are in 1.0 L of a 4.8 M Mg(NO3)2 solution?

Calculate the molarity of each of the following solutions: a. 0.400 mole of urea (CH4N2O) in 250.0 mL of solution b. 1.78 mole of NH4C2H3O2 in 1.000 L of solution c. 2.00 mole of methanol (CH 3OH) in 5.000 L of solution

A solution containing equal masses of glycerol (C3H8O3) and water has a density of 1.10 g/mL. Calculate the molarity of glycerol in the solution.

A chemist adds 470.0 mL of a 8.8 x 10-5 mM silver(II) oxide (AgO) solution to a reaction flask. Calculate the mass in micrograms of silver(II) oxide chemist has added to the flask. Round your answer to 2 significant digits.

What is the molarity of a solution made by dissolving 2.5 g of NaCl in enough water to make 725 mL of solution? (a) 0.059 M (b) none of these (c) 0.0094 M (d) 0.31 M (e) 0.20 M

You have 500 mL of a 5.0 M solution of nitric acid HNO3 (63.01 g/mol) dissolved in water. How many grams of nitrogen does the solution contain? (i) 160 g (ii) 150 g (iii) 35 g (iv) 2.5 g

How many grams of solute are present in 385 mL of 0.240 M KBr?

Sodium hydroxide is extremely soluble in water. At a certain temperature, a saturated solution contains 543 g of NaOH(s) per liter of solution. Calculate the molarity of this saturated NaOH(aq) solution.

A chemist prepares a solution of aluminum chloride (AICI 3) by measuring out 24.6 g of aluminum chloride into a 250. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's aluminum chloride solution. Be sure your answer has the correct number of significant digits.

Calculate the molarity of 0.900 mol of Na2S in 1.75 L of solution.Calculate the molarity of 21.7 g of MgS in 773 mL of solution.

If 5.91 g of CuNO, is dissolved in water to make a 0.790 M solution, what is the volume of the solution?

Calculate the mass of NaCl in a 35-mL sample of a 1.6 M NaCl solution. Express your answer using two significant figures.

What NaCl concentration results when 229 mL of a 0.640 M NaCl solution is mixed with 452 mL of a 0.220 M NaCl solution?

Calculate the volume in liters of a 2.0 x 10-5 µmol/L zinc oxalate solution that contains 900 mg of zinc oxalate (ZnC2O4). Be sure your answer has the correct number of significant digits.

In the laboratory you dissolve 17.7 g of sodium acetate in a volumetric flask and add water to a total volume of 125 ml. What is the molarity of the solution? What is the concentration of the sodium cation? What is the concentration of the acetate anion?

A student weighs out a 7.62 g sample of AlI3, transfers it to a 100. mL volumetric flask, adds enough water to dissolve it and then adds water to the 100. mL tick mark. What is the molarity of aluminum iodide in the resulting solution? Molarity = _____ M

How many grams of solute are needed to prepare each of the following solutions? a. 1.000 L of 0.215 M NaClb. 250.0 mL of 0.145 M CuSO4C. 500.0 mL of 0.410 M CH3OH

If 4.99 g of CuNO3 is dissolved in water to make a 0.190 M solution, what is the volume of the solution?

Calculate the molarity of 125.0 mL of a solution that is 0.92 % by mass NaCl. Assume the density of the solution is the same as pure water.

Calculate the number of moles of solute present in 245 mL of 1.50 M HNO3(aq) a. 0.368 mol b. 0.0368 mol c. 0.194 mol d. 0.0194 mol e. 0.245 mol

How many grams of cobalt(II) sulfate, CoSO4, must be dissolved to prepare 300 mL of a 0.125 M aqueous solution of the salt?

Calculate the volume in milliliters of a 3.67 mol/L calcium bromide solution that contains 225 mmol of calcium bromide (CaBr2). Be sure your answer has the correct number of significant digits.

What mass of ammonium acetate would be required to prepare 1405 mL of 1.20 M NH4C2H3O2 solution? (a) 1.30 x 102 g (b) none of these (c) 2.19 g (d) 90.3 g (e) 65.9 g

Sodium hydroxide is extremely soluble in water. At a certain temperature, a saturated solution contains 561 g of NaOH(s) per liter of solution. Calculate the molarity of this saturated NaOH(aq) solution.

How many grams of NaOH would be needed to make 200. mL of 0.600 M solution? molecular weight of NaOH = 40.0 g/mol

Calculate the molarity of the two solutions. a) 0.550 mol of NaOH in 2.70 L of solution. b) 12.7 g of NaCl in 715 mL of solution.

Calculate the molarity of 0.400 mol of Na2S in 1.30 L of solution. Calculate the molarity of 21.1 g of MgS in 979 mL of solution.

When a 1.00 L sample of water from the surface of the Dead Sea (which is more than 400 meters below sea level and much saltier than ordinary seawater) is evaporated, 1.70 x 102 grams of MgCl2 are recovered. What is the molarity of MgCl 2 in the original sample?

Enter your answer in the provided box. An aqueous solution that is 10.0 percent sulfuric acid (H2SO4) by mass has a density of 1.307 g/mL. Determine the molarity of the solution.

15.45g of CuNOs is dissolved in water to make a 0.710 M solution, what is the volume of the solution?

Part A How many grams of ethanol, CH3CH2OH, should you dissolve in water to make 1.60 L of vodka (which is an aqueous solution that is 6.86 M ethanol)? Expess your answer with the appropriate units.Part B Using the density of ethanol (0.789 g/mL), calculate the volume of ethanol you need to make 1.60 L of vodka. Express your answer with the appropriate units.

If 3.31 g of CuNO3 is dissolved in water to make a 0.220 M solution, what is the volume of the solution?

How many mL of a 0.212 M aqueous solution of chromium(II) chloride, CrCl2, must be taken to obtain 3.05 grams of the salt?

What is the concentration (in M) of methanol in an aqueous solution if dissolving 1.25 mol of methanol in water produces a 10.0 L solution? A. 125 x 10-1 M B. 1.25 x 100 M C. 1.25 x 101 M D. 1.25 x 102 M

What is the molarity of 0.73 mol of NaCI in enough water to make 3.0 L of solution?

0.755 M H2SO4 solution reacts with 55.0 mL of 2.50 M KOH solution. Given: 2KOH (aq) + H2SO4 (aq) → 2H2O (l) + K2SO4 (aq). How many moles of KOH are there?

How many moles of NaOH are present in 31.5 mL of 0.300 M NaOH?

Sodium hydroxide is extremely soluble in water. At a certain temperature, a saturated solution contains 571 g of NaOH(s) per liter of solution. Calculate the molarity of this saturated NaOH(aq) solution.

Calculate: How many grams of solid AgNO3 will be needed to prepare 250. mL of a 0.0500 M solution? How many grams of vitamin C (C6H8O6) would be contained in 45.0 mL of a 1.60 M solution? How many moles of HCl is contained in 450. ml of 3.5 M solution?

Write an equation to solve for moles, given molarity and volume. Then write an equation to convert X moles to grams, assuming a molar mass of Z grams per mole. Write an equation to solve for moles in terms of M (molarity) and V (volume in liters):

A 365 ml can of soda pop contains 45 g of sucrose (C12H22O11) What is the molarity of the solution with respect to sucrose Express your answer using two significant figures.

How many grams of solute are present in 885 mL of 0.310 M KBr?

How many moles of solute are in 2.38 L of 0.18M Na2SO4? The molar mass of Na2SO4 is 142 g/mol. (a) 0.43 mol Na2SO4 (b) 0.076 mol Na2SO4 (c) 13.2 mol Na2SO4 (d) 61 mol Na2SO4

The average adult human male has a total blood volume of 4.9 L.If the concentration of sodium ion in this average individual is 0.136 M, what is the mass of sodium ion circulating in the blood? Express your answer using two significant figures.

Calculate the volume in milliters of a 1.43M sodium nitrate solution that contains 75.0 mmol of sodium nitrate (NaNO3). Be sure your answer has the correct number of significant digits.

If 8.23 g of CuNO3 is dissolved in water to make a 0.690 M solution, what is the volume of the solution?

Calculate the volume in liters of a 9.1 x 10 -4 mmol/L magnesium fluoride solution that contains 2.00 mol of magnesium fluoride (MgF2). Be sure your answer has the correct number of significant digits.

What is the molarity of the Al3+ ions when 0.25 mol of aluminum nitrate, Al(NO3), is dissolved in enough water to make 3.0 L of solution?

How many grams of solute are present in 465 mL of 0.780 M KBr?

Calculate the molarity of 0.950 mol of Na2S in 1.20 L of solution. Calculate the molarity of 29.9 g of MgS in 741 mL of solution.

Enter your answer in the provided box.An aqueous solution that is 30.0 percent sulfuric acid (H2SO4) by mass has a density of 1.307 g/mL. Determine the molarity of the solution.

The mass of acetic acid (CH3COOH, molecular mass = 60.06 g/mol) needed to prepare 125 mL of a 0.450 M solution isa. 56.3 gb. 0.937 gc. 1.07 gd. 3.38 g

In the laboratory you dissolve 13.2 g of manganese(II) chloride in a volumetric flask and add water to a total volume of 500 mL. What is the molarity of the solution? What is the concentration of the manganese (II) cation? What is the concentration of the chloride anion?

What is the volume of 0.85 mol of benzene (C 6H6) at 20.7 degree C? The density of benzene is 0.879 g/mL.

Calculate the volume in liters of a 1.3 mol/L aluminum chloride solution that contains 200. g of aluminum chloride (AICl3). Round your answer to 2 significant digits.

Part A Calculate the molarity of a solution that contains 0.155 mol ZnCl2 in exactly 190 mL of solution. Part B How many moles of HNO3 are present in 35.0 mL of a 4.40 M solution of nitric acid? Part C How many mililiters of 6.20 M NaOH solution are needed to provide 0.300 mol of NaOH?

A 93.60 mL solution was made by dissolving 9.00 g of phosphoric acid (H 3PO4, 97.994 g/mol)) in water. Calculate the molarity of this solution. Answer:

How many grams of solute are present in 115 mL of 0.790 M KBr?

A student weighs out a 2.29 g sample of FeSO4, transfers it to a 100. mL volumetric flask, adds enough water to dissolve it and then adds water to the 100. mL tick mark. What is the molarity of iron(II) sulfate in the resulting solution? Molarity = _____ M

Be sure to answer all parts. Determine how many grams of each of the following solutes would be needed to make 3.30 x 102 mL of a 0.100 M solution. (a) cesium iodide (Csl): (b) sulfuric acid (H2SO4): (c) sodium carbonate (Na2CO3): (d) potassium dichromate (K2Cr2O): (e) potassium permanganate (KMnO4):

Part AHow many moles of Ba(OH)2 are present in 175 mL of 0.200 M Ba(OH)2? Express your answer with the appropriate units. Part BHow many moles of HNO3 are present if 3.50 x 10-2 mol of Ba(OH)2 was needed to neutralize the acid solution? Express your answer with the appropriate units. Part CWhat is the concentration of HNO3 if 7.00 x 10-2 mol are present in 735 mL of the solution? Express your answer with the appropriate units.

5.5 M NaCI represents 5.5 moles of NaCI in 1 L of water.a. Trueb. False

If 2.23g of CuNO3 is dissolved in water to make a 0.490 M solution, what is the volume of the solution?

How many grams of solute are present in 655 mL of 0.380 M KBr?