Ch.4 - Reactions in Aqueous Solution
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Problem 103a
(a) By titration, 15.0 mL of 0.1008 M sodium hydroxide is needed to neutralize a 0.2053-g sample of a weak acid. What is the molar mass of the acid if it is monoprotic?
Problem 103b
(b) An elemental analysis of the acid indicates that it is composed of 5.89% H, 70.6% C, and 23.5% O by mass. What is its molecular formula?
- A fertilizer railroad car carrying 129,840 L of commercial aqueous ammonia (30% ammonia by mass) tips over and spills. The density of the aqueous ammonia solution is 0.88 g/cm³. What mass of citric acid, C₆H₈O₇ (which contains three acidic protons), is required to neutralize the spill?
Problem 105
Problem 105a
Suppose you have 5.00 g of powdered magnesium metal, 1.00 L of 2.00 M potassium nitrate solution, and 1.00 L of 2.00 M silver nitrate solution. a. Which one of the solutions will react with the magnesium powder?
Problem 106c
A sample of 7.75 g of Mg(OH)2 is added to 25.0 mL of 0.200 𝑀 HNO3. c. How many moles of Mg(OH)2,HNO3, and Mg(NO3)2 are present after the reaction is complete?