University:
Missouri State University
Course:
CHM 160 | General Chemistry I
Academic year:

2020
Views:

347

Pages:

2
Author:

Hallie Randolph

KEY Name______________ Worksheet: Molarity Molarity: quantitative • a _______________ description of solution concentration. M • Abbreviated _______________ moles of solute Molarity = ________________ liters of solution Problems: Show all work and circle your final answer. 1. To make a 4.00 M solution, how many moles of solute will be needed if 12.0 liters of solution are required? 4.00 M = moles of solute 12.0 L moles of solute = 48.0 mol 2. How many moles of sucrose are dissolved in 250 mL of solution if the solution concentration is 0.150 M? 1L = 0.25 L 1000 mL moles of solute 0.150 M = moles of solute = 0.038 mol 0.25 L ? L = 250 mL × 3. What is the molarity of a solution of HNO3 that contains 12.6 grams HNO3 in 1.0 L of solution? ? mol HNO3 = 12.6 g HNO3 × M= 1 mol HNO3 = 0.200 mol HNO3 63.0 g HNO3 0.200 mol HNO3 = 0.200 M 1.0 L 4. How many grams of potassium nitrate are required to prepare 0.250 L of a 0.700 M solution? 0.700 M = moles of solute 0.250 L moles of solute = 0.175 mol ? g KNO3 = 0.175 mol KNO3 × 101.1 g KNO3 = 17.7 g KNO3 1 mol KNO3 5. 125 cm3 of solution contains 3.5 moles of solute. What is the molarity of the solution? ? g KNO3 = 0.175 mol KNO3 × M= 101.1 g KNO3 = 17.7 g KNO3 1 mol KNO3 3.5 mol = 28 M 0.125 L 6. Which solution is more concentrated? Solution “A” contains 50.0 g of CaCO3 in 500.0 mL of solution. Solution “B” contains 6.0 moles of H2SO4 in 4.0 L of solution. SHOW WORK! ? mol CaCO3 = 50.0 g CaCO3 × “A”: ? L = 500.0 mL × “B”: M= 1 mol CaCO3 = 0.500 mol CaCO3 100.0 g CaCO3 1L = 0.500 L 1000 mL 6.0 mol = 1.5 M 4.0 L M= 0.500 mol = 1.00 M 0.500 L “B” is more concentrated: 1.5 M 7. How many liters of solution can be produced from 2.5 moles of solute if a 2.0 M solution is needed? 2.0 M = 2.5 moles liters of solution liters of solution = 1.25 L = 1.3 L 8. What would be the concentration of a solution formed when 1.00 g of NaCl are dissolved in water to make 100.0 mL of solution? ? mol = 1.00 g NaCl × ? L = 100.0 mL × 1 mol NaCl = 0.0171 mol NaCl 58.5 g NaCl 1L = 0.1000 L 1000 mL M= 0.0171 mol = 0.171 M 0.1000 L