6. Silver nitrate, AgNO3, can be used to test for the presence of chloride ions

Question

6. Silver nitrate, AgNO3, can be used to test for the presence of chloride ions in solution, because it readily forms a precipitate of AgCl. What volume of 2.0 M AgNO, will be required to react with 50.0 mL of a 0.10 M HCI solution? AgNO3(aq) + HCI(aq)- AgCl(s) + HNO3(aq) 7. Write the correct equilibrium constant expression for the following reaction: H,(g) +1,(g) 2HI(g) If the equilibrium concentrations are [HI] -1.0 M, [H2]-0.10 M, [Ch]-0.10 M, what is the value of the equilibrium constant? Are reactants or products favoured? 8. List the acid, base, conjugate acid, and conjugate base for the following reaction: HOCl (ag)H20OC (a) HO* (a 9. What are the products of an acetate ion, CH3Co, reacting with water? 10. If the pH of a coffee sample is 5.15, what is the hydronium ion concentration in the coffee? 11. Given an OH concentration of 1.0 x 10 M, calculate the H,0' concentration and then identify the solution as acidic, basic, or neutral.

Explanation / Answer

6.

AgNO3 (aq.) + HCl (aq.) -----------> AgCl (s) + HNO3 (aq.)

Moles of HCl = molarity * volume in L = 0.10 * 50.0 / 1000 = 0.00500 mol

From the balanced equation,

1 mol of HCl needs 1 mol of AgNO3.

SO, 0.00500 mol of HCl needs 0.00500 mol of AgNO3

Volume of AgNO3 needed = moles / molarity = 0.00500 / 2.0 = 0.00250 L = 2.50 mL of AgNO3

7.

Kc = [HI]2 / [H2][I2]

Kc = (1.0)2 / (0.1)(0.1)

Kc = 100

8.

Acid = HOCl

Base = H2O

Conjugate acid = H3O+

Conjugate base = OCl-

9.

CH3COO- (aq.) + H2O (l) = CH3COOH (aq.) + OH- (aq.)

Acetic acid and hydroxide ion

10.

pH = 5.15

- Log[H3O+] = 5.15

[H3O+] = 7.08 * 10-6 M

11.

[OH-] = 10-6 M

[H3O+] = 1.0 * 10-14 / 10-6

[H3O+] = 1.0 * 10-8 M

Since [H3O+] < 10-7, the solution is basic.

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