In a solution, the solute is the smaller portion that is being dissolved by the solvent, the larger portion usually in the form of H_{2}O. Molarity is the term used to describe the solubility of the solute within the solvent in the creation of a solution.

**Molarity Formula **

Molarity serves as the bridge between moles and volume. It is the concentration of a solution represented as moles of solute per liter of solution:

This would mean a solution that is 0.10 M NaCl:

Although moles per liter are the traditional units for molarity, you can also use mg/mL because it is proportionally equivalent.

**Molarity Calculations**

From the molarity formula, you can calculate volume, grams or the moles of solute.

To calculate molarity from mass (in grams, milligrams, etc.) and volume (milliliters, liters, microliters, etc.) we do the following.

**PRACTICE 1: **Find the molarity from 25.0 g NaCl in 500 mL solution.

**STEP 1:** Convert the grams given into moles given.

**STEP 2: **Convert milliliters into liters.

**STEP 3: **To find the molarity of the solution plug in the moles and liters calculated from Steps 1 and 2.

Now we must calculate the mass from volume and concentration.

**PRACTICE 2: **Find the grams of NaCl from 50.0 mL of 0.120 M NaCl.

**STEP 1:** Rearrange the molarity formula in order to isolate the moles.

**STEP 2:** Convert the milliliters into liters.

**STEP 3:** Multiply liters and molarity together to isolate the moles of the compound.

**STEP 4:** Convert the moles into grams.

Finally here's how you calculate the volume from mass and concentration.

**PRACTICE 3: **Find the volume (in mL) of 0.110 M NaCl from 2.50 moles NaCl.

**STEP 1:** Rearrange the molarity formula in order to isolate the liters.

**STEP 2:** Divide moles by molarity to isolate the liters of the compound.

**STEP 3:** Convert liters into millimeters.

**Osmolarity**

Ionic molarity or osmolarity represents the molarity of dissolved ions in a solution. For example, if you were asked how to calculate the osmolarity of 0.200 M KNO_{3}.

** STEP 1**: Break the ionic compound into its ions.

** STEP 2**: Now calculate the osmolarity of the solution with its equation.

**Dilutions**

Another common idea related to molarity deals with the dilution of stock solutions. In a dilution a concentrated solution is made more diluted by adding water directly to it.

**After Molarity **

Eventually you will do calculations that connect molarity to problems with density, molarity vs molality, mole fraction, mass fraction or percent.

Beyond these calculations that deal directly with the molarity formula you can bring in stoichiometry. This brings in more complex problems dealing with solution chemistry, acid base titration, pH and pOH.

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

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

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

(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

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?

Carminic acid, a naturally occurring red pigment extracted from the cochineal insect, contains only carbon, hydrogen, and oxygen. It was commonly used as a dye in the first half of the nineteenth century. It is 53.66% C and 4.09% H by mass. A titration required 18.02 mL of 0.0406 M NaOH to neutralize 0.3602 g carminic acid. Assuming that there is only one acidic hydrogen per molecule, what is the molecular formula of carminic acid?

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

A 25.00-mL sample of hydrochloric acid solution requires 24.16 mL of 0.106 M sodium hydroxide for complete neutralization. What is the concentration of the original hydrochloric acid 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 10.00-mL sample of vinegar, an aqueous solution of acetic acid (HC 2H3O2), is titrated with 0.5062 M NaOH, and 16.58 mL is required to reach the equivalence point.a. What is the molarity of the acetic acid?

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

A 10.00-mL sample of vinegar, an aqueous solution of acetic acid (HC 2H3O2), is titrated with 0.5062 M NaOH, and 16.58 mL is required to reach the equivalence point.b. If the density of the vinegar is 1.006 g/cm 3, what is the mass percent of acetic acid in the vinegar?

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

Citric acid, which can be obtained from lemon juice, has the molecular formula C6H8O7. A 0.250-g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?

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

What volume of 0.0200 M calcium hydroxide is required to neutralize 35.00 mL of 0.0500 M nitric acid?

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

A 30.0-mL sample of an unknown strong base is neutralized after the addition of 12.0 mL of a 0.150 M HNO3 solution. If the unknown base concentration is 0.0300 M, give some possible identities for the unknown base.

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.

The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of 204.22 g/mol. In the titration, 34.67 mL of the sodium hydroxide solution was required to react with 0.1082 g KHP. Calculate the molarity of the sodium hydroxide.

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.

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?

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

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.

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?

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 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?

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

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?

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.

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.

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

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