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To 150 mL of water was added 0.18 moles of ammonia (NH3 Kb= 2.3 x 10-5) calcula…

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Wize University Chemistry Textbook > Acids and Bases

Autoionization of Water (Kw)

5 Activities

Wize University Chemistry Textbook > Acids and Bases

Base Equations (Kb, pKb)

1 Activity

To 150 mL of water was added 0.18 moles of ammonia (NH3 Kb= 2.3 x 10-5) calculate the pH.
More Autoionization of Water (Kw) Questions:
Concentration
A solution of LiOH is made by mixing an unknown amount of LiOH with 1 L of water. The pOH is measured to be 3.65, what is the concentration of LiOH?
MW Li: 7 g/mol
MW O: 16 g/mol
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10-10) solution
Diet cola drinks have a pH of about 3.0, while milk has a pH of about 7.0. How many times greater is the H3O+ concentration in diet cola than in milk?
Acids and Bases: Ka
The following occurs when HCl is placed in water:
HCl <----> H+ + Cl-
The Ka for this reaction is known to be Ka = 5.64 once it reaches equilibrium. At equilibrium, 1.35 x 10-7 M of HCl and 1.2 M of Cl- can be found. What is the pH of the solution at equilibrium?
Acids and Bases: pH
100 mL100\ mL of a 0.5 M0.5\ M solution of Hydrochloric acid (HCl\rm HCl) was added to 48 mL48\ mL of a 0.410 M0.410\ M solution of sodium benzoate (C6H5COONa\rm C_6H_5COONa) the conjugate base of benzoic acid (C6H5COOH\rm C_6H_5COOH Ka=6.6×10−5\rm K_a = 6.6 \times 10^{-5}). Calculate the pH\rm pH of the resulting solution.
An aqueous solution only contains a 0.050 M in a weak base. Which of the following statements would be true about the solution?
Lactic acid, shown below, is added to many beverages, including some sour beers. What is the pH of a 0.050M lactic acid solution in 0.50M hydrochloric acid? (Ka for lactic acid=1.38x10-4)
What is the hydroxide ion (OH-) concentration of a solution with a pH of 6.1?
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10-10) solution
Diet cola drinks have a pH of about 3.0, while milk has a pH of about 7.0. How many times greater is the H3O+ concentration in diet cola than in milk?
What is the pH of a solution prepared by mixing 50 mL of a 0.10 M HCl solution with 150 mL of pure water?
What is the pH of a 1.1M solution of nitrous acid (HNO2). The Ka of nitrous acid is 7.2 x 10-4
Diet cola drinks have a pH of about 3.0, while milk has a pH of about 7.0. How many times greater is the H3O+ concentration in diet cola than in milk?
Concentration
A solution of LiOH is made by mixing an unknown amount of LiOH with 1 L of water. The pOH is measured to be 3.65, what is the concentration of LiOH?
MW Li: 7 g/mol
MW O: 16 g/mol
pH: Neutralization
A student adds 11.6 mL of a 3.7M KOH solution, to 29 mL of a 1.4 M HCl. What is the final pH after the addition?
To 4.00 L of water was added 100 mg of HF (6.6 x 10-4). What is the pH?
CH3COOH is a weak acid with a Ka of 1.8 x 10-5. In what pH range would you most likely an aqueous solution of Na(CH3COO).
Acids and Bases: Henderson Hasselbalch
To a solution of acetic acid (Ka=1.8×10−5\rm K_a = 1.8 \times 10^{-5}) was added 0.1 mol of NaOH\rm NaOH. After the addition of NaOH\rm NaOH the volume was 1.4L and the pH\rm pH was 5.2.
a) This solution a buffer? (True/False)
b) Calculate the number of moles of acetic acid that were originally in solution. Report your answer in moles to three significant figures. Do not include units in the answer field
What is the pH of a solution made by mixing 22g of NaOH in 3.1 L of water?
Molecular formula: Concentration
A solution of HBr has a pOH of 12.2, what is the [H+] concentration?
What is the pH of a solution of 0.1 M sodium acetate (NaCH3CO2) given that the Ka for acetic acid is 1.8×10−5?
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10-10) solution
To a 90 mL90\ mL of 0.17 M0.17\ M of HF\rm HF is added 25 mL25\ mL of 0.06 M0.06\ M NaOH\rm NaOH. The KaK_a of HF\rm HF is 7.2×10−47.2 \times 10^{-4}. Calculate the pH\rm pH of the solution.
What is the pH of pure, neutral water at 37°C? At 37°C, Kw = 2.4x10-14.
A student titrated 10.00 mL of 0.10 M sodium acetate (CH3COONa) with HCℓ and determined that 10.00 mL of HCℓ was needed to reach the equivalence point. At equivalence, what is the expected pH?
Ka of CH3COOH = 1.8×10-5
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10-10) solution
What is the pH of a solution prepared by mixing 50 mL of a 0.10 M HCl solution with 150 mL of pure water?
The equilibrium constant for the auto-ionization of water at 10 °C is 3.0 x 10-15. What is the concentration of H3O+ ions in pure water at this temperature?
If the pH of pure water is 6.80 at 37 °C, calculate Kw pOH and [OH- ] at this temperature.
Equilibrium: Auto-ionization of water
Given the equilibrium information for water below, what is the concentration of hydroxide ions in a solution of 1.5 M HCl?
2 H2O (l) ⇌ H3O+ (aq) + OH- (aq), Kc = 1x10-14 at 20oC
Equilibrium: ICE Tables and Auto-ionization of Water
Given the equilibrium information for water below, what is the concentration of hydroxide ions in water?
2 H2O (l) ⇌ H3O+ (aq) + OH- (aq), Kc = 1x10-14 at 20oC
If the pH of pure water is 6.80 at 37 °C, calculate Kw pOH and [OH- ] at this temperature.
The compound fluoroacetic acid (shown), has a pKa value of 2.59. What is pKb of its conjugate base?
A solution of [CH3NH3][CH3COO] is made in an undergraduate laboratory. Use the information below to predict the acidity of the solution.
CH3COOH: Ka = 1.8 x 10-5
CH3NH3+: Ka = 2.3 x 10-11
Auto-ionization of Water: pH
If the pH of pure water is 6.80 at 37 °C, calculate Kw pOH and [OH- ] at this temperature.
If an answer has an exponent (ex. 1.6x103), input it as: 1.6e3
The equilibrium constant for the auto-ionization of water at 10 °C is 3.0 x 10-15. What is the concentration of H3O+ ions in pure water at this temperature?
More Base Equations (Kb, pKb) Questions:
Acids and Bases: Base equations
CH3NH3 is a weak base. When mixed with water, we see the following reaction:
CH3NH3 + H2O <----> CH3NH4+ + OH-
Once the reaction reaches equilibrium, Kb was found to be 1.07 x 10-3. If the reaction at equilibrium contains 2.5 M CH3NH3 and 0.37 M CH3NH4+, how much OH- is in solution?
Consider the following reaction in water:
NaOH <----> Na+ + OH-
This reaction has a Kb of 1 x 10-10 and a pOH of 3. If there is 1 M of NaOH at equilibrium, what is the concentration of Na+ in solution?
An aqueous solution only contains a 0.050 M in a weak base. Which of the following statements would be true about the solution?
Consider the weak bases below and their Kb values:
C6H7OKb=1.3×10−10C_6H_7O \hspace{48pt}K_b=1.3 \times 10^{-10}
C2H5NH2Kb=5.6×10−4C_2H_5NH_2 \hspace{30pt}K_b=5.6 \times 10^{-4}
Ammonia(NH3) is a weak base, Kb = 1.8 x 10-5 and benzoic acid (C6H5CH2O-) is a weak acid, Ka = 6.3 x 10-5. A solution of ammonium benzoate (NH4)(C6H5CH2O-) is:
Triemethylamine (N(CH3)3) is a base (pKb=4.19) used in a variety of organic reactions. It can also be used as an effective Lewis base due to it's small steric profile.
if a solution of [N(CH3)3H]2[SO4]is dissolved in neutral water the pH will be,
Strength of Acids and Bases
What is the strongest acid below? What is the weakest acid?
Strongest acid:
Cl3CCOOH
Weakest acid:
HCN
Acids and Bases: Base Equations
Consider the weak bases below and their Kb values:
C6H7OKb=1.3×10−10C2H5NH2Kb=5.6×10−4C5H5NKb=1.7×10−9\begin{alignedat}{} &C_6H_7O &&K_b = 1.3\times10^{-10}\\ &C_2H_5NH_2 &&K_b = 5.6\times10^{-4}\\ &C_5H_5N &&K_b = 1.7\times10^{-9} \end{alignedat}
Arrange the conjugate acids of these weak bases in order of increasing acid strength.