Clicker Questions Chapter 16 Barbara Mowery York College

A Brønsted–Lowry acid is a proton donor. a proton acceptor. an electron-pair donor. d. an electron-pair acceptor. Answer: a

A Brønsted–Lowry acid is a proton donor. a proton acceptor. an electron-pair donor. d. an electron-pair acceptor. Answer: a

A Brønsted–Lowry base is a proton donor. a proton acceptor. an electron-pair donor. d. an electron-pair acceptor. Answer: b

A Brønsted–Lowry base is a proton donor. a proton acceptor. an electron-pair donor. d. an electron-pair acceptor. Answer: b

A Lewis acid is a proton donor. a proton acceptor. an electron-pair donor. d. an electron-pair acceptor. Answer: d

A Lewis acid is a proton donor. a proton acceptor. an electron-pair donor. d. an electron-pair acceptor. Answer: d

A Lewis base is a proton donor. a proton acceptor. an electron-pair donor. d. an electron-pair acceptor. Answer: c

A Lewis base is a proton donor. a proton acceptor. an electron-pair donor. d. an electron-pair acceptor. Answer: c

Which of the following is the conjugate base of HPO42−? d. HPO32− Answer: c

Which of the following is the conjugate base of HPO42−? d. HPO32− Answer: c

Which species is amphiprotic? H3PO4 H2PO41− PO43− d. None of these Answer: b

Which species is amphiprotic? H3PO4 H2PO41− PO43− d. None of these Answer: b

Which of the following is the conjugate acid of SO42−? H2SO4 HSO41− SO32− d. H3SO4+ Answer: b

Which of the following is the conjugate acid of SO42−? H2SO4 HSO41− SO32− d. H3SO4+ Answer: b

The stronger the acid, the (X) its conjugate base The stronger the acid, the (X) its conjugate base. Acids and bases react to form their (Y) conjugates. X = stronger, Y = stronger X = stronger, Y = weaker X = weaker, Y = stronger d. X = weaker, Y = weaker Answer: d

The stronger the acid, the (X) its conjugate base The stronger the acid, the (X) its conjugate base. Acids and bases react to form their (Y) conjugates. X = stronger, Y = stronger X = stronger, Y = weaker X = weaker, Y = stronger d. X = weaker, Y = weaker Answer: d

For a conjugate acid–base pair, Kw = Ka ___ Kb. + −  d. / Answer: c

For a conjugate acid–base pair, Kw = Ka ___ Kb. + −  d. / Answer: c

The value of the ion-product constant for water is 10−7. 10−14. 10+7. d. impossible to determine without additional information. Answer: c

The value of the ion-product constant for water is 10−7. 10−14. 10+7. d. impossible to determine without additional information. Answer: c

What is the pH of a 0.0200 M aqueous solution of HBr? 1.00 1.70 2.30 d. 12.30 Answer: b

What is the pH of a 0.0200 M aqueous solution of HBr? 1.00 1.70 2.30 d. 12.30 Answer: b

What is the pH of a 0.0400 M aqueous solution of KOH? 12.60 10.30 4.00 d. 1.40 Answer: a

What is the pH of a 0.0400 M aqueous solution of KOH? 12.60 10.30 4.00 d. 1.40 Answer: a

What is the pH of a 0.0200 M aqueous solution of HF? The Ka of HF is 6.8  10−4. 1.70 2.43 3.17 d. 12.30 Answer: b

What is the pH of a 0.0200 M aqueous solution of HF? The Ka of HF is 6.8  10−4. 1.70 2.43 3.17 d. 12.30 Answer: b

A 0.30 M acid solution has a pH of 1.85. What is the % ionization? 21 % 16 % 6.2 % 4.7 % Answer: d

A 0.30 M acid solution has a pH of 1.85. What is the % ionization? 21 % 16 % 6.2 % 4.7 % Answer: d

What is the pH of a 0. 100 M aqueous solution of NH3 What is the pH of a 0.100 M aqueous solution of NH3? The Kb of NH3 is 1.8  10−5. 2.87 4.74 9.26 d. 11.13 Answer: d

What is the pH of a 0. 100 M aqueous solution of NH3 What is the pH of a 0.100 M aqueous solution of NH3? The Kb of NH3 is 1.8  10−5. 2.87 4.74 9.26 d. 11.13 Answer: d

What is the pH of a 0.0400 M aqueous solution of KF? The Ka of HF is 6.8  10−4. 2.28 2.43 6.12 d. 7.88 Answer: d

What is the pH of a 0.0400 M aqueous solution of KF? The Ka of HF is 6.8  10−4. 2.28 2.43 6.12 d. 7.88 Answer: d

What is the pH of a 1.0  10−8 M aqueous solution of HBr? 6.00 6.96 7.04 d. 8.00 Answer: b

What is the pH of a 1.0  10−8 M aqueous solution of HBr? 6.00 6.96 7.04 d. 8.00 Answer: b

Which of the following is not a weak base? NH3 NH2OH F− OH− Answer: d

Which of the following is not a weak base? NH3 NH2OH F− OH− Answer: d

Which of the following correctly lists the acids in order of decreasing strength? HClO2 > HClO > HBrO > HIO HClO > HBrO > HIO > HClO2 HIO > HBrO > HClO > HClO2 d. HClO2 > HIO > HBrO > HClO Answer: a

Which of the following correctly lists the acids in order of decreasing strength? HClO2 > HClO > HBrO > HIO HClO > HBrO > HIO > HClO2 HIO > HBrO > HClO > HClO2 d. HClO2 > HIO > HBrO > HClO Answer: a

Aqueous metal ions behave as Lewis acids because they can readily accept electrons in their vacant d orbitals. can readily donate electron pairs from their outermost p orbitals. attract electrons from the water molecules they are dissolved in. d. are attracted to the electronegative oxygen atoms in the solvent. Answer: a

Aqueous metal ions behave as Lewis acids because they can readily accept electrons in their vacant d orbitals. can readily donate electron pairs from their outermost p orbitals. attract electrons from the water molecules they are dissolved in. d. are attracted to the electronegative oxygen atoms in the solvent. Answer: a