chap10 chem

If 20.0 mL (0.0200 L) of a 0.234 M H2SO4 solution is required to titrate 45.6 mL (0.0456 L) of a NaOH solution, what is the molarity of the NaOH solution? Balanced equation: H2SO4(aq) + 2NaOH(aq) → Na2SO4(aq) + 2H2O(l)

0.205 M

Calculate the [H3O+] of an aqueous solution of vinegar with [OH-] = 1.0 x 10-11 M. Given: Kw = [H3O+][OH-] = 1.0 x 10-14

1.0 x 10-3 M

What is the pH of a solution with [OH-] = 1 × 10-4 M? (Given: Kw = [H3O+][OH-] = 1.0 x 10-14)

10.0

What is the pH of a solution with [OH-] = 1 × 10-4 M? (Given: Kw = [H3O+][OH-] = 1.0 x 10-14)

10.0

If the [H3O+] is 4.95 x 10-12 M, what is the pH?

11.305

Given that the pH of a solution is 6.7, what is the [H3O+]?

2 x 10-7 M

Given the following balanced equation: H3PO4(aq) + 3LiOH(aq) → Li3PO4(aq) + 3H2O(l) A solution of 0.785 M H3PO4 is used to titrate 27.5 mL (0.0275 L) of a LiOH solution. If 32.0 mL (0.0320 L) of the H3PO4 solution is required, what is the molarity of the LiOH solution?

2.74 M

Given the following balanced equation: H3PO4(aq) + 3LiOH(aq) → Li3PO4(aq) + 3H2O(l) A solution of 0.785 M H3PO4 is used to titrate 27.5 mL (0.0275 L) of a LiOH solution. If 32.0 mL (0.0320 L) of the H3PO4 solution is required, what is the molarity of the LiOH solution?

2.74 M

If [H3O+] = 2.65 x 10-4 M, what is [OH-]? Given: Kw = [H3O+][OH-] = 1.00 x 10-14

3.77 x 10-11 M

Given that the pH of a solution is 4.62, what is the [OH-]? (Kw = [H3O+][OH-] = 1.0 x 10-14) (Hints: [H3O+] = 1 x 10-pH; The number of decimal places in the pH value gives the number of significant figures in [H3O+].)

4.2 × 10-10 M

Given that the pH of a solution is 4.62, what is the [OH-]? (Kw = [H3O+][OH-] = 1.0 x 10-14)

4.2 × 10-10 M

Calculate the pH of a solution with [H3O+] = 6.7 x 10-8 M. (Hints: pH = - log[H3O+]; The number of significant figures in [H3O+] gives the number of decimal places in the pH value.)

7.17

Which of the following statements correctly describes a buffer solution?

A buffer contains a weak acid and the salt of its conjugate base

Which of the following statements correctly describes a buffer solution?

A buffer contains a weak acid and the salt of its conjugate base.

What is a buffer?

A buffer is a solution that maintains pH by neutralizing added acid or base.

What would the products of the reaction between calcium carbonate (CaCO3) and hydrochloric acid (HCl) be?

CO2(g), CaCl2(aq), and H2O(l)

In the following equation, identify which reactant is the acid (H+ donor) and which reactant is the base (H+ acceptor), according to the Bronsted-Lowry concept. CO32-(aq) + H2O(l) ⇄ HCO3-(aq) + OH-(aq)

CO32- is the base, and H2O is the acid.

Which of the following constitutes a buffer system?

H2CO3 (a weak acid) and NaHCO3 (salt containing HCO3-, the conjugate base of H2CO3)

If the products of a neutralization reaction are MgBr2(aq) and H2O(l), what are the chemical formulas of the reactant acid and base?

HBr and Mg(OH)2

Which acid has the strongest conjugate base?

HCN

In the following equation, identify which reactant is the acid (H+ donor) and which reactant is the base (H+ acceptor), according to the Bronsted-Lowry concept. HCN(aq) + SO42-(aq) ⇄ CN-(aq) + HSO4-(aq)

HCN is the acid, and SO42- is the base.

Identify the conjugate acid-base pairs in the following equation: HCN(aq) + NO2-(aq) ⇄ HNO2(aq) + CN-(aq)

HCN/CN- and HNO2/NO2-

Which set of chemicals is an acid-base conjugate pair?

HClO2 and ClO2-

Which of the following is a strong acid

HClO4

Which of the following is a strong acid?

HClO4

Which of the following compounds is an acid?

HF

Which of the following compounds is an acid?

HI

In the following equation, identify which reactant is the acid (H+ donor) and which reactant is the base (H+ acceptor), according to the Bronsted-Lowry concept. HI(aq) + H2O(l) → H3O+(aq) + I-(aq)

HI is the acid, and H2O is the base.

Write the formula of the acid containing the nitrate ion.

HNO3

Which acid has the weakest conjugate base?

HSO4-

Which of the following is a buffer solution?

NH3 (a weak base) and NH4Cl (salt containing NH4+, the conjugate acid of NH3)

What is the rule for naming an acid formed from an oxygen-containing polyatomic anion with the name ending in ate?

No prefix is used before the name of the polyatomic anion, but its ate ending is changed to ic acid.

What is the rule for naming an acid formed from an oxygen-containing polyatomic anion with the name ending in ite?

No prefix is used before the name of the polyatomic anion, but its ite ending is changed to ous acid.

Given the following reaction: H3PO4(aq) + H2O(l) ⇄ H2PO4-(aq) + H3O+(aq) What happens when more H2PO4-(aq) is added to the solution?

The equilibrium shifts to the left, producing more H3PO4 (aq).

Consider the buffer system of nitrous acid (HNO2) and its salt, NaNO2, which provides the conjugate base, NO2-. HNO2(aq) + H2O (l) ⇄ H3O+ (aq) + NO2-(aq) How does the buffer react when some acid is added?

The nitrite ion (NO2-) of the buffer reacts with the acid.

What is the rule for naming an acid formed from a simple nonmetal anion, the latter having the name ending in ide?

The prefix hydro is used before the name of the nonmetal, and its ide ending is changed to ic acid.

Given the following reaction: NH3(aq) + H2O(l) ⇄ NH4+(aq) + OH-(aq) Which change will cause a shift towards the product side?

addition of NH3(aq)

What would the name of the acid containing the bromate ion be?

bromic acid

Write the name of the acid containing the chlorate ion.

chloric acid

Which substance is a base when dissolved in water, as defined by Arrhenius?

magnesium hydroxide

CO32-(aq) + H2O(l) ⇄ HCO3-(aq) + OH-(aq) Which change will cause an increase in the rate of the reverse reaction?

removal of CO32-(aq)

What is the name of the acid containing the sulfite ion?

sulfurous acid