Which classification is correct for the reaction?

H₂PO₄⁻(aq) + H₂O(l) → HPO₄²⁻(aq) + H₃O⁺(aq)

Which is an acid-base conjugate pair?

Which of the following is correct?

Which species produced by the successive dissociations of phosphoric acid, H₃PO₄, are amphiprotic?

Which species acts as a Lewis and Brønsted–Lowry base?

Which species behave as Brønsted–Lowry bases in the following reaction?

H₂SO₄ + HNO₃ H₂NO₃⁺ + HSO₄^-

Which is a conjugate Brønsted–Lowry acid-base pair?

Which are acid-base pairs according to the Brønsted‒Lowry theory?

I. HNO3/NO−3

II. H3O+/OH−

III. HCOOH/HCOO−

Which of the following is an example of a Lewis acid–base reaction, but not a Brønsted–Lowry acid–base reaction?

Which row correctly describes

1.0 moldm⁻³ NaOH(aq)?

What is the Brønsted–Lowry conjugate base of H₂PO⁻⁴?

Which descriptions are correct for both a Brønsted–Lowry acid and a Lewis acid?

Consider the equilibrium below.

CH₃CH₂COOH(aq) + H₂O(l) ⇌ CH₃CH₂COO⁻(aq) + H₃O⁺(aq)

Which species represent a conjugate acid-base pair?

Which is not a conjugate acid-base pair?

What is the conjugate base of H₂CO₃ according to the Brønsted-Lowry theory?

Which species behave as Brønsted-Lowry acids in the following reversible reaction?

H₂PO₄⁻(aq) + CN⁻(aq) ⇌ HCN(aq) + HPO₄²⁻(aq)

What is the formula of the conjugate base of the hydrogenphosphate ion, HPO₄²⁻?

Which are definitions of an acid according to the Brønsted-Lowry and Lewis theories?

According to the Brønsted-Lowry theory, how does each species act in the equilibrium below?

CH₃COOH + H₂SO₄ ⇌ CH₃COOH₂+ + HSO₄⁻

With which do most acids react?

I. sodium hydrogen carbonate

II. magnesium

III. calcium sulfate

What are the products of the reaction between sulfuric acid and sodium hydrogen carbonate?

Which react with dilute sulfuric acid?

I. Cu

II. CuO

III. CuCO₃

What occurs when solid sodium hydrogen carbonate reacts with aqueous sulfuric acid?

A student carried out a titration to determine the concentration of an acid and found that his value had good precision but poor accuracy. Which process explains this outcome?

Which gas in the atmosphere causes the pH of unpolluted rain to be approximately 6?

Which compound reacts with calcium oxide, CaO?

Which solutions have a pH less than 7?

I. Na₂CO₃ (aq)

II. [Fe(H₂O)₆]Cl₃ (aq)

III. (NH₄)₂SO₄ (aq)

If 20 cm³ samples of 0.1 moldm⁻³ solutions of the acids below are taken, which acid would require a different volume of 0.1 moldm⁻³ sodium hydroxide for complete neutralization?

Which solution is basic at 25 °C?

K_w = 1.0 × 10⁻¹⁴

What is the pH of 0.001 mol dm⁻³ NaOH (aq)?

What is the pH of a solution in which the hydroxide ion concentration is 1 × 10⁻¹¹ mol dm⁻³ at 298 K?

K_w = 1 × 10⁻¹⁴ at 298 K

What will happen if the pressure is increased in the following reaction mixture at equilibrium?

CO₂ (g) + H₂O (l) ⇌ H⁺ (aq) + HCO₃⁻ (aq)

10.0 cm³ of an aqueous solution of sodium hydroxide of pH = 10 is mixed with 990.0 cm³ of distilled water. What is the pH of the resulting solution?

Which statement is incorrect for a 0.10 mol dm^–3 HCOOH solution?

What is the pH of 1.0 × 10⁻³ mol dm⁻³ sodium hydroxide, NaOH(aq)?

K_w = 1.0 × 10⁻¹⁴

10.0 cm³ of a solution of a strong acid with a pH of 3 is added to a volumetric flask and the total volume is made up to 1.00 dm³ by adding distilled water. The resulting solution is then thoroughly mixed.

What is the pH of the diluted solution?

A solution of 50 cm³ hydrochloric acid has a pH of 4. What is the final pH if 450 cm³ of water is added?

A solution of acid HX has a pH = 1 and a solution of acid HY has a pH = 3. Which statement must be correct?

What is the pH of the solution formed when 10 cm³ of HCl (aq) with pH 1.0 is added to 990 cm³

of water?

The pH of a solution changes from pH=2 to pH=5. What happens to the concentration of the hydrogen ions during this pH change?

An example of a strong acid solution is perchloric acid, HClO₄, in water. Which statement is correct for this solution?

What is the correct expression for the ionic product constant of water, K_w?

What is the order of increasing pH for the following solutions of the same concentration?

Which statement is correct?

Which 1.0 moldm^–3 solution has the highest pH?

Which compound is a strong acid?

A student adds 0.3 g of magnesium metal to equal volumes of hydrochloric acid and ethanoic acid of the same concentrations in separate flasks. Which statement is correct?

Which group of three compounds contains only weak acids and bases?

Which list contains only strong bases?

Which products would be formed when hydrochloric acid reacts with magnesium oxide?

Which group of three compounds contains only weak acids and bases?

The table below shows data for the K_a and pK_b values for some acids and bases at 298 K. Which two formulas represent the weakest acid and the weakest base in the table?

Which salts will dissolve in water to give solutions with a pH above 7?

I. Na₂CO₃

II. CH₃COONa

III. Na₂SO₄

Which 0.10 moldm⁻³ solution would have the highest conductivity?

A solution of acid A has a pH of 1 and a solution of acid B has a pH of 2. Which statement must be correct?

Which of the following are weak acids in aqueous solution?

I. CH₃COOH

II. H₂CO₃

III. HCl

For equal volumes of 1.0 moldm⁻³ solutions of hydrochloric acid, HCl(aq), and methanoic acid, HCOOH(aq), which statements are correct?

I. HCl dissociates more than HCOOH

II. HCl is a better electrical conductor than HCOOH

III. HCl will neutralize more NaOH than HCOOH

When equal volumes of four 0.1 moldm⁻³ solutions are arranged in order of increasing pH (lowest pH first), what is the correct order?

Which list contains only strong acids?

Which is not a source of oxides of sulfur and nitrogen?

What is the major reason why the pH of unpolluted rain is less than 7?

Which of the following gases does not result in acid deposition?

Which pH value is that of an aqueous solution of carbon dioxide?