chemistry

 

4. Assuming that each single-replacement reaction occurs, predict the products and write each balanced chemical equation.

Li + MgSO₄ →?

 

NaBr + Cl₂ →?

 

14. Assuming that each double-replacement reaction occurs, predict the products and write each balanced chemical equation.

Sn(OH)₂ + FeBr₃ →?

 

CsNO₃ + KCl →?

 

16. Use the solubility rules to predict if each double-replacement reaction will occur and, if so, write a balanced chemical equation.

Na₂CO₃ + Sr(NO₂)₂ →?

 

(NH₄)₂SO₄ + Ba(NO₃)₂ →?

 

 

Chapter 11.1 4, 6, 12

4. A solution is prepared by combining 10.3 g of Hg(ℓ) and 45.0 g of Ag(s). Identify the solute and solvent.

 

 

6. Use Table 11.2 “Solubilities of Some Ionic Compounds” to decide if a solution containing 0.000092 g of AgCl per 100 g of H₂O is unsaturated, saturated, or supersaturated.

 

12. Which solvent is NaOH more likely soluble in—CH₃OH or C₆H₆?

 

 

 

Chapter 11.2 4, 6, 8

 

4. What is the molarity of a solution made by dissolving 332 g of C₆H₁₂O₆ in 4.66 L of solution?

 

6.How many moles of NH₄Br are present in 88.9 mL of a 0.228 M solution?

 

8. What volume of 3.99 M H₂SO₄ is needed to obtain 4.61 mol of H₂SO₄?

 

 

Chapter 11.3   2, 6, 8, 10

 

2. What quantity remains constant when you dilute a solution?

 

6. If 12.00 L of a 6.00 M HNO₃ solution needs to be diluted to 0.750 M, what will be its final volume?

 

8. If 1.00 L of an LiOH solution is boiled down to 164 mL and its initial concentration is 0.00555 M, what is its final concentration?

 

10. How much water must be added to 1.55 L of 1.65 M Sc(NO₃)₃(aq) to reduce its concentration to 1.00 M?

 

 

Chapter 11.4 12

 

12. What volume of 1.000 M Na₂CO₃ will react with 342 mL of 0.733 M H₃PO₄?

3Na₂CO₃ + 2H₃PO₄ → 2Na₃PO₄ + 3H₂O + 3CO₂

 

 

 

Chapter 11.7 10

10. For sanitary reasons, water in pools should be chlorinated to a maximum level of 3.0 ppm. In a typical 5,000gal pool that contains 21,200 kg of water, what mass of chlorine must be added to obtain this concentration?