Molarity and Solution Stoichiometry

Which solution has the highest molarity when 25.0 grams of the solute is dissolved in 250.0 milliliters of solution?

NaCl

What is the molarity of a solution prepared from 15.0 grams of Al(NO3)3 in 300.0 milliliters of solution?

0.235 M Al(NO3)3

What is the molarity of a solution prepared from 34.5 grams of NaCl in 250.0 milliliters of solution?

2.36 M NaCl

Which solution has the lowest molarity when 25.0 grams of the solute is dissolved in 250.0 milliliters of solution?

KNO3

Assume 0.18 L of a 1.8 M solution of potassium chloride, KCl, reacts with a 1.25 M solution of lead (II) nitrate, Pb(NO3)2, to produce lead (II) chloride, PbCl2, and potassium nitrate, KNO3. The problem requires that you determine the volume of lead (II) nitrate, Pb(NO3)2, needed for the reaction to occur.

2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)

1 mol Pb(NO3)2 / 2 mol K Cl

Assume 0.18 L of a 5.0 M solution of lead (II) nitrate, Pb(NO3)2, reacts with a 2.6 M solution of sodium phosphate, Na3PO4, to produce lead (II) phosphate, Pb3(PO4)2, and sodium nitrate, NaNO3. The problem requires that you determine the volume of sodium phosphate, Na3PO4, needed for the reaction to occur.

3 Pb(NO3)2(aq) + 2 Na3PO4(aq) → Pb3(PO4)2(s) + 6 NaNO3(aq)

5.0 mol Pb(NO3)2/ 1L Pb (NO3)2

Assume 0.12 L of a 2.0 M solution of hydrochloric acid, HCl, reacts with a 0.25 M solution of calcium hydroxide, Ca(OH)2, to produce calcium chloride, CaCl2, and water, H2O. The problem requires that you determine the volume of calcium hydroxide, Ca(OH)2, needed for the reaction to occur.

2 HCl(aq) + Ca(OH)2(aq) → CaCl2(aq) + 2 H2O(l)

1 L Ca (OH)2 / 0.25 mol Ca(OH)2

Which solution has the lowest molarity when 25.0 grams of the solute is dissolved in 250.0 milliliters of solution?

AlCl3

Assume 0.25 L of a 1.8 M solution of aluminum sulfate, Al2(SO4)3, reacts with a 4.2 M solution of sodium hydroxide, NaOH, to produce sodium sulfate, Na2SO4, and aluminum hydroxide, Al(OH)3. The problem requires that you determine the volume of sodium hydroxide, NaOH, needed for the reaction to occur.

Al2(SO4)3(aq) +6 NaOH(aq) → 3 Na2SO4(aq) + 2 Al(OH)3(s)

1.8 mol Al2 (SO4)3 / 1L Al2 (SO4)3

A 17.50 mL sample of a 0.150 M solution of H3PO4 reacts with excess Ba(OH)2. What mass of H2O is produced in the reaction?

2 H3PO4(aq) + 3 Ba(OH)2(aq) → Ba3(PO4)2(aq) + 6 H2O(l)

0.142 g H2O

Assume 0.15 L of a 0.10 M solution of iodine, I2, reacts with a 0.33 M solution of vitamin C or ascorbic acid, C6H8O6, to produce dehydroascorbic acid, C6H6O6, and hydrogen iodide, HI. The problem requires that you determine the volume of vitamin C, C6H8O6, needed for the reaction to occur.

C6H8O6(aq) + I2(aq) → C6H6O6(aq) + 2 HI(aq)

1 mol C6H8O6 / 1 mol I2

Which solution has the highest molarity when 25.0 grams of the solute is dissolved in 250.0 milliliters of solution?

LiCl

What is the molarity of a solution having 1.4 moles of sodium chloride, NaCl, and a volume of 525 mL?

Assume 0.55 L of a 1.6 M solution of sodium sulfate, Na2SO4, reacts with a 0.75 M solution of barium chloride, BaCl2, to produce sodium chloride, NaCl, and barium sulfate, BaSO4. The problem requires that you determine the volume of barium chloride, BaCl2, needed for the reaction to occur.

Na2SO4(aq) + BaCl2(aq) → 2 NaCl(aq) + BaSO4(s)

1 L BaCL2 / 0.75 mol BaCl2

Assume 0.12 L of a 2.0 M solution of potassium hydroxide, KOH, reacts with a 2.8 M solution of calcium nitrate, Ca(NO3)2, to produce calcium hydroxide, Ca(OH)2, and potassium nitrate, KNO3. The problem requires that you determine the volume of calcium nitrate, Ca(NO3)2, needed for the reaction to occur.

2 KOH(aq) + Ca(NO3)2(aq) → Ca(OH)2(s) + 2 KNO3(aq)

1 mol Ca(NO3)2 / 2 mol KOH

What is the molarity of a solution prepared from 19.7 grams of MgCl2 in 275 milliliters of solutions?

0.753 M MgCl2

Assume 0.35 L of a 2.5 M solution of potassium bromide, KBr, reacts with a 3.2 M solution of chlorine, Cl2, to produce potassium chloride, KCl, and bromine, Br2. The problem requires that you determine the volume of chlorine, Cl2, needed for the reaction to occur.

2 KBr(aq) + Cl2(aq) → 2 KCl(aq) + Br2(l)

2.5 mol KBr / 1L KBr

A 20.00 mL sample of a 0.250 M solution of HCl reacts with excess Ba(OH)2. What mass of H2O is produced in the reaction?

2 HCl(aq) + Ba(OH)2(aq) → BaCl2(aq) + 2 H2O(l)

0.0901 g H2O

What is the molarity of a solution prepared from 29.2 grams of KNO3 in 425 milliliters of solutions?

0.680 M KNO3

A 35.00 mL sample of a 0.200 M solution of H3PO4 reacts with excess NaOH. What mass of H2O is produced in the reaction?

H3PO4(aq) + 3 NaOH(aq) → Na3PO4(aq) + 3 H2O(l)

0.378 g H2O

0.378 g H2OA 25.00 mL sample of a 0.100 M solution of HCl reacts with excess NaOH. What mass of H2O is produced in the reaction?

HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

0.0451 g H2O

Assume 0.23 L of a 1.8 M solution of lead (II) nitrate, Pb(NO3)2, reacts with a 1.4 M solution of sodium chloride, NaCl, to produce lead (II) chloride, PbCl2, and sodium nitrate, NaNO3. The problem requires that you determine the volume of sodium chloride, NaCl, needed for the reaction to occur.

Pb(NO3)2(aq) + 2 NaCl(aq) → PbCl2(s) + 2 NaNO3(aq)

1 L NaCl / 1.4 mol NaCl

What is the molarity of a solution having 2.0 moles of glucose, C6H12O6, and a volume of 850 mL?

2.4 M C6H12O6

Assume 0.42 L of a 0.95 M solution of nickel (II) chloride, NiCl2, reacts with a 1.5 M solution of sodium hydroxide, NaOH, to produce nickel (II) hydroxide, Ni(OH)2, and sodium chloride, NaCl. The problem requires that you determine the volume of sodium hydroxide, NaOH, needed for the reaction to occur.

NiCl2(aq) + 2 NaOH(aq) → Ni(OH)2(s) + 2 NaCl(aq)

2 mol NaOH / 1 mol NiCl2

Assume 0.38 L of a 2.8 M solution of magnesium chloride, MgCl2, reacts with a 2.3 M solution of silver (I) nitrate, AgNO3, to produce silver (I) chloride, AgCl, and magnesium nitrate, Mg(NO3)2. The problem requires that you determine the volume of silver (I) nitrate, AgNO3, needed for the reaction to occur.

MgCl2(aq) + 2 AgNO3(aq) → 2 AgCl(s) + Mg(NO3)2(aq)

1 L AgNO3 / 2.3 mol AgNO3

Assume 0.25 L of a 1.5 M solution of silver (I) nitrate, AgNO3, reacts with a 1.2 M solution of magnesium chloride, MgCl2, to produce silver (I) chloride, AgCl, and magnesium nitrate, Mg(NO3)2. The problem requires that you determine the volume of magnesium chloride, MgCl2, needed for the reaction to occur.

2 AgNO3(aq) + MgCl2(aq) → 2 AgCl(s) + Mg(NO3)2(aq)

1.5 mol AgNO3 / 1 L AgNO3