Subjects

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Molarity | 23 mins | 0 completed | Learn Summary |

Solution Stoichiometry | 22 mins | 0 completed | Learn |

Solubility Rules | 7 mins | 0 completed | Learn Summary |

Net Ionic Equations | 21 mins | 0 completed | Learn Summary |

Electrolytes | 19 mins | 0 completed | Learn Summary |

Redox Reaction | 32 mins | 0 completed | Learn Summary |

Balancing Redox Reactions | 22 mins | 0 completed | Learn |

Activity Series | 19 mins | 0 completed | Learn |

Chemical Quantities Additional Problems | 46 mins | 0 completed | Learn |

Additional Practice |
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Redox Reactions |

Calculate Oxidation Number |

Additional Guides |
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Dilution |

Net Ionic Equation |

Oxidation Reduction (Redox) Reactions |

Oxidation Number |

Types of Chemical Reactions |

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.

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

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 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

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

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

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

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 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

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.

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

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

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

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

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 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

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

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

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

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

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).

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

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

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.

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

(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?

(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?

(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?

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

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

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?

(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?

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

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

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.

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.

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.

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.

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

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

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.

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?

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?

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?

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.

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

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

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

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 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

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

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

How many moles of Nal are in 23.0 mL of a 0.250 M solution?A. 0.250 moles NalB. 5.75 moles NalC. 0.00575 moles NalD. 0.0920 moles NalE. 10.9 moles Nal

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

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.

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

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

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 ?

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.

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

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

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?

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 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.

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.

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

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?

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

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

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.

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

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

What is the concentration (M) of lithium ions in 4.57 L of a 2.35 M Li 3P solution?a. 45.0 Mb. 14.1 Mc. 2.35 Md. 7.05 Me. 99.0 M

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?

The molecular weight of ethanol (C2H5OH) is 46.1 and the density of absolute (100%) ethanol = 0.79 g/mLThe 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?

What is the total molar concentration of ions in each of the following solutions, assuming complete dissociation? A 0.685 M solution of K2CO3

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.

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 the chemist has added to the flask. Round your answer to 2 significant digits.

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

Calculate the mass of KI in grams required to prepare 5.00 x 10 2 mL of a 1.5 M 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

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.

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

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.

A student sets up and solves the following equation to solve a problem in solution stoichiometry. Fill in the missing part of the student's equation. (4.2 ) (0.30 L) (115.40 g/mol) = 1.5 x 10 2 g

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?

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.

The molecular weight of ethanol (C2H5OH) is 46.1 and the density of absolute (100%) ethanol = 0.79 g/mLa) 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.

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?

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

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?

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