Exam 2 Flashcards by Mar Morimoto

Predict pH for the compound, KBr

Approximately equal to 7

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Predict pH for the compound, NH4Br

Less than 7

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Predict pH for the compound, NaF

Greater than 7

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Buffer or not a buffer?

HClO4 and NaClO4

Not a buffer

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Buffer or not a buffer?

H2CO3 and Na2CO3

Buffer

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Buffer or not a buffer?

NH4Cl and NH3

Buffer

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Buffer or not a buffer?

HF and NaOH

Not a buffer

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Given an acetate buffer that is a mixture with 0.25M acetic acid CH3COOH and 0.25M sodium acetate NaCH3COO. Ka = 1.8 x 10^-5.

(a) Calculate the pH of the buffer
(b) Calculate the pH after 1.0mL of 0.25M NaOH is added to 100.0mL of this buffer
(c) Calculate the pH after 1.0mL of 0.25M HCl is added to 100.0mL of this buffer

(a) pH = 4.74
(b) pH = 4.74
(c) pH = 4.74

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A Bronsted-Lowry base is defined as

A proton acceptor

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Which of the following is a stronger acid?

CH3COOH or C2H5COOH

CH3COOH

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Which of the following is a stronger acid?

H2CO3 or H2SO3

H2SO3

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Calculate the hydronium ion concentration in an aqueous solution with a pOH of 9.85 at 25°C.

7.1 x 10^-5

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Calculate the concentration of H3O+ in a solution that contains 5.5 x 10^-5 M OH- at 25°C. Identify the solution as acidic, basic, or neutral.

1.8 x 10^-10 M, basic

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Type the formula for the conjugate base of the following acid: (HPO4)2-

(PO4)3-

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Type the formula for the conjugate acid of the following base: (CO3)2-

HCO3-

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Given the following weak acid equilibrium reaction:

HA (aq) + H2O (l) H3O+ (aq) + A- (aq)

Calculate the pH of 3.12M HA solution. Given Ka = 6.5 x 10^-8

pH = 3.35

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Write a chemical equation for the following:

HNO3 reacts with KOH

H3O+ (aq) + OH- (aq) –> 2 H2O (l)

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Write a chemical equation for the following:

HCl reacts with NH3

H3O+ (aq) + NH3 ↔ H2O (l) + NH4+ (aq)

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Write a chemical equation for the following:

CH3COOH reacts with NaOH

CH3COOH (aq) + OH- (aq) –> CH3COO- + H2O (l)

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Write a chemical equation for the following:

NaHSO3 reacts with Na2CO3

HSO3- (aq) + (CO3)2- (aq) ↔ (SO3)2- (aq) + HCO3- (aq)

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Acetate buffers are used in biochemical studies of enzymes and other chemical components of cells to prevent pH changes that might change the biochemical activity of these compounds.

(a) Calculate the pH of an acetate buffer that is a mixture with 0.10M acetic acid and 0.10M sodium acetate.
(b) Calculate the pH after 1.0mL of 0.10M NaOH is added to 100.0mL of this buffer.
(c) Calculate the pH after 1.0mL of 0.10M HCl is added to 100.0mL of this buffer.

(a) pH = 4.74
(b) pH = 4.75
(c) pH = 4.74

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The carbonate buffer system in the blood uses the following reaction:

H2CO3 (aq) ↔ HCO3 (aq) + H3O+ (aq)

The concentration of carbonic acid, H2CO3, is approximately 0.0012M and the concentration of the hydrogen carbonate ion, HCO3-, is around 0.024M. Calculate the pH of blood.

pH = 7.66

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Calculate the equilibrium concentrations of all ions of barium sulfate in a 0.020M sodium sulfate solution. The solubility product constant for barium sulfate is 1.1 x 10^-10.

[Ba2+] = 5.5 x 10^-9 M

[(SO4)3-] = 0.020 M

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A titration is carried out for 25.00mL of 0.100M HCl (strong acid) with 0.100M of a strong base NaOH. Calculate the pH after the following volumes of NaOH are added:

(a) 0.00mL
(b) 12.50mL
(c) 25.00mL
(d) 37.50mL

(a) pH = 1.00
(b) pH = 1.48
(c) pH = 7.00
(d) pH = 12.30

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Calculate the pH at the following points in a titration of a 40.0 mL of 0.100M barbituric acid (Ka = 9.8x10^-5) with 0.100M KOH. (a) No KOH added (b) 20.0mL of KOH added (c) 39.0mL of KOH added (d) 40.0mL of KOH added (e) 41.0mL of KOH added

(a) pH = 2.51 (b) pH = 4.01 (c) pH = 5.60 (d) pH = 8.34 (e) pH = 11.09

Write the conjugate acid formulas of the following base: CN-

HCN

Write the conjugate acid formulas of the following base: ClO4-

HClO4

Write the conjugate acid formulas of the following base: HSO3-

H2SO3

Write the conjugate base formulas of the following base: HF

F-

Write the conjugate base formulas of the following base: HNO3

NO3-

Write the conjugate base formulas of the following base: HSO3-

(SO3)2-

Write the following acid-base reactions between: HSO3- acts as an acid and H2O as a base

HSO3- + H2O ↔ SO32- + H3O+

Write the following acid-base reactions between: (CO3)2- acts as a base and H2O as an acid

CO32- + H2O ↔ HCO3- + OH-

Write the following acid-base reactions between: NH4+ acts as an acid and (CO3)2- as a base

NH4+ + CO32- ↔ NH3 + HCO3-

Identify the stronger acid: | HClO4 or HClO

HClO4

Identify the stronger acid: | HClO4 or HBrO4

HClO4

Identify the stronger acid: | HCl or HF

HCl

Identify the stronger acid: | CH3COOH or C2H5COOH

CH3COOH

Determine the pH of a 0.0516M nitric acid.

pH = 1.29

Given the following chemical reaction between a weak acid, HA, and water: HA (aq) + H2O (l) ↔ A- (aq) + H3O+ (aq) Calculate the Ka of a 0.546M of HA solution with a pH of 4.56.

Ka = 1.39 x 10^-9

Acetic acid, CH3COOH is the main component of vinegar, apart from water. CH3COOH (aq) + H2O (l) ↔ CH3COO- (aq) + H3O+ (aq) Determine the pH in a 0.25M acetic acid solution (Ka = 1.8 x 10^-5)

pH = 2.68

Given the following equilibrium reaction of NH3: NH3 (aq) + H2O (l) ↔ NH4+ (aq) + OH- (aq) Determine the pH in a 1.25M NH3 solution (Ka = 5.6x 10^-10)

pH = 11.67

Identify the strongest acid: HFO4 HFO HFO3 HFO2

HFO4

Calculate the pOH of a solution that contains 2.4 x 10^-5 M H3O+ at 25°C.

pOH = 9.38

Determine the pOH of a 0.00598M HClO4 solution.

pOH = 11.777

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25°C.

7.1 x 10^-5 M

Determine the pH in a 0.235M NaOH solution.

pH = 13.37

What is the pH of a 0.100M NH3 solution that has Kb = 1.8 x 10^-5? The equation for the dissociation of NH3 is: NH3 (aq) + H2O (l) ↔ NH4+ (aq) + OH- (aq)

pH = 11.13

What is the conjugate acid of HCO3-?

H2CO3

Calculate the hydronium ion concentration in an aqueous solution with a pOH of 9.85 at 25°C.

7.1 x 10^-5 M

The stronger the acid, the _____ the conjugate base.

weaker

Which of the following solutions would have the highest pH? Assume that they are all 0.10M in acid at 25°C. The acid is followed by its Ka value. HCHO2, 1.8 x 10^-4 HClO2, 1.1 x 10^-2 HNO2, 4.6 x 10^-10 HCN, 4.9 x 10^-10 HF, 3.5 x 10^-4

HCN, 4.9 x 10^-10

Calculate the hydroxide ion concentration in an aqueous solution with a pOH of 9.85 at 25°C.

1.4 x 10^-10 M

What is the conjugate base of H2PO4-?

(HPO4)2-

Which of the following is an Arrhenius base? KBr CH3CO2H RbOH CH3OH More than one of these compounds is an Arrhenius base

RbOH

Calculate the pH of a 0.800M NaCH3CO2 solution. Ka for acetic acid, CH3CO2H, is 1.8 x 10^-5.

pH = 9.32

Identify the products that are in equilibrium with NH3 and H2O.

NH4+ and OH-

Identify the strong diprotic acid. HNO3 H2SO4 H2CO3 H2SO3

H2SO4

A 900.0mL sample of 0.18M HClO4 is titrated with 0.27M LiOH. Determine the pH of the solution after the addition of 300.0mL of LiOH.

pH = 7.00

Calculate the pH of a buffer that is 0.032M HF and 0.032M NaF. The Ka for HF is 3.5 x 10^-4.

pH = 3.46

Calculate the pH of a buffer that is 0.060M HF and 0.030M KF. The Ka for HF is 3.5 x 10^-4.

pH = 3.16

The molar solubility of Ag2S is 1.26 x 10^-16M in pure water. Calculate the Ksp for Ag2S.

8.00 x 10^-48M

When titrating a weak monoprotic acid with NaOH at 25°C, the (a) Titration will require more moles of acid than base to reach the equivalence point. (b) pH will be equal to 7 at the equivalence point (c) pH will be greater than 7 at the equivalence point (d) Titration will require more moles of base than acid to reach the equivalence point (e) pH will be less than 7 at the equivalence point

A 500.0mL sample of 0.18M HClO4 is titrated with 0.27M CsOH. Determine the pH of the solution after the addition of 250.0mL of CsOH.

pH = 1.52

Calculate the pH of a 0.080M carbonic acid solution, H2CO3 (aq), that has the stepwise dissociation constants: Ka1 = 4.3 x 10^-7 Ka2 = 5.6 x 10^-11

pH = 3.73

The molar solubility of Ba3(PO4)2 is 8.89 x 10^-9M in pure water. Calculate the Ksp for Ba3(PO4)2.

6.00 x 10^-39 M

A 100.0mL sample of 0.20M HF is titrated with 0.10M KOH. Determine the pH of the solution after the addition of 300.0mL of KOH. The Ka of HF is 3.5 x 10^-4.

pH = 12.40

Determine the molar solubility of MgCO3 in pure water. Ksp (MgCO3) = 6.82 x 10^-6

2.61 x 10^-3 M

A 200.0mL sample of 0.18M HClO4 is titrated with 0.36M NaOH. Determine the pH of the solution before the addition of any NaOH.

pH = 0.74

A 1.50L buffer solution is 0.250M in HF and 0.250M in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of NaOH. The Ka for HF is 3.5 x 10^-4.

pH = 3.57

Calculate the pH of a buffer that is 0.020M HF and 0.040M NaF. The Ka for HF is 3.5 x 10^-4.

pH = 3.76

Determine the molar solubility of AgI in pure water. Ksp (AgI) = 8.51 x 10^-17

9.22 x 10^-9 M

A 100.0mL sample of 0.20M HF is titrated with 0.10M NaOH. Determine the pH of the solution after the addition of 200.0mL of NaOH. The Ka of HF is 3.5 x 10^-4.

pH = 8.14

A 200.0mL sample of 0.180M HClO4 is titrated with 0.270M KOH. Determine the pH of the solution after the addition of 150.0mL of KOH.

pH = 12.1

A 600.0mL sample of 0.20M HF is titrated with 0.10M NaOH. Determine the pH of the solution after the addition of 600.0mL of NaOH. The Ka of HF is 3.5 x 10^-4.

pH = 3.46

Determine the pH of a 0.22M NaF solution at 25°C. The Ka of HF is 3.5 x 10^-5.

pH = 8.90

A 900.0mL sample of 0.18 M HClO4 is titrated with 0.27M NaOH. Determine the pH of the solution after the addition of 270.0mL of NaOH.

pH = 1.12

Determine the molar solubility of PbSO4 in pure water. Ksp (PbSO4) = 1.82 x 10^-8.

1.35 x 10^-4 M

A Bronsted-Lowry acid is defined as

A proton donor

An Arrhenius acid produces _____ in solution

H3O+

An Arrhenius base produces _____ in solution

OH-

What are the strong acids?

HCl HBr HI HNO3 H2SO4 HClO4

What are the strong bases?

LiOH NaOH KOH Ca(OH)2 Sr(OH)2 Ba(OH)2

Ka = product/reactant As product increases, Ka _____.

Increases

Ka = product/reactant As product decreases, Ka _____.

Decreases

Which one is the stronger acid? HNO3 or HNO2

HNO3

Which one is the stronger acid? H2SO4 or H3PO4

H2SO4

Which one is the stronger acid? HCl or H2CO3

HCl

If [H3O+] = 2.6 x 10^-5M, what is [OH]eq?

3.8 x 10^-10 M

Calculate the pH and pOH of a solution with [H3O+]eq = 1.0 x 10^-5 M.

pH = 5.0 pOH = 9.0

Calculate the pH and pOH of a 0.0125M KOH.

pH = 12.10 pOH = 1.90

The pKa of benzoic acid is 4.20. Calculate Ka, Kb, and pKb.

pKb = 9.80 Ka = 6.31 x 10^-5 Kb = 1.58 x 10^-10

If you see a strong acid, write it as _____.

H3O+

If you see a strong base, write it as _____.

OH-

Exam 2 Flashcards

(94 cards)