Assignment:
Question 1. A solution is prepared by dissolving 10.8g ammonium sulfate in enough water to make 100.0mL of stock solution. A 10.00mL sample of this stock solution is added to 50.00mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.
Question 2. One of the most commonly used white pigments in paint is a compound of titanium and oxygen that contains 59.9% Ti by mass. Determine the empirical formula of this compound.
Question 3. A compound that contains only nitrogen and oxygen is 30.4% N by mass; the molar mass of the compound is 92g/mol. What is the empirical formula of the compound? What is the molecular formula of the compound?
Question 4. Mercury and bromide will react with each other to produce mercury (II) bromide:
Hg(l) + Br2(l) → HgBr2(s)
a) What mass of HgBr2 can be produced form the reaction of 10.0g Hg and 9.00g Br2? What mass of which reagent is left unreacted?
b) What mass of HgBr2 can be produced form the reaction of 5.00mL mercury (density = 13.6g/mL) and 4.00mL bromine (density = 3.10g/mL)?
Question 5. Consider the following unbalanced reaction:
Ca3(PO4)2 + H2SO4 → CaSO4 + H3PO4
What masses of calcium sulfate and phosphoric acid can be produced from the reaction of 1.0kg calcium phosphate with 1.0kg concentrated sulfuric acid (98% H2SO4 by mass)?
Question 6. What volume of each of the following acids will react completely with 50.00mL of 0.200M NaOH?
a) 0.100 M HCl
b) 0.150 M HNO3
c) 0.200 M HC2H3O2 (1 acidic hydrogen)
Provide complete and step by step solution for the question and show calculations and use formulas.