250. mL of an 8.0 μM solution of the salt of a weak acid (NaD) is...
250. mL of an 8.0 μM solution of the salt of a weak acid (NaD) is added to 250. mL of water. The Ka of the acid HD is 2.5x10-9 . What is the pH of the final solution?
Write out a chemical equation:
__________ + __________ <-------------> ___________ + ___________
Write out an equilibrium chart:
| I | ||||
| C | ||||
| E |
Calculate the pH of this solution once equilibrium has been reached:
e. Rank the acids HA, HB, HC, and HD from the problems above in increasing acid strength.
Homework Answers
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250. mL of an 8.0 μM solution of the salt of a weak acid (NaD)
is...
1.A 1.76 M solution of a weak acid HA is found to have a pH of...
1.A 1.76 M solution of a weak acid HA is found to have a pH of 2.22 Determine Kg of the acid Determine Kb of its conjugate base, A Determine [OH'] in a 2.00 M solution of the weak acid's sodium salt, NaA M Determine the pH of a 2.00 M solution of the sodium salt, NaA 2.The pH of a 1.93 M solution of a weak base B is measured to be 10.82 Determine Kp of the base Determine...
A student wishes to prepare a buffer solution at pH = 5.60. Which of these weak...
A student wishes to prepare a buffer solution at pH = 5.60. Which of these weak acids (HA, HB and HC) should he/she choose: HA (pKa = 2.57), HB (pKa = 5.36), or HC (pKa = 8.59)? Select one: a. Only HA b. Only HC c. Only HB d. HA or HB e. None of HA, HB or HC
39. A solution of a weak monoprotic acid, HA (0.50 M), and its potassium salt, KA...
39. A solution of a weak monoprotic acid, HA (0.50 M), and its potassium salt, KA (0.75 M), has a measured pH = 4.88. What is the value of Ka for this acid?
50.0 mL sample of the weak acid the concentration of the weak acid = 0.15 M...
50.0 mL sample of the weak acid
the concentration of the weak acid = 0.15 M
25 mL of the week acid into 100 mL beaker
titrated this solution of 0.21 M NaOH
moles of weak acid = 3.75*10^-3
moles of NaOH = moles of week acid
c) How many milliliters of the NaOH are required to neutralize the sample of weak acid? d) How many moles of NaOH have been added at one half of the volume in part...
50 ml of 0.100M solution of a weak acid HB titrated with NaOH. Calculate ph at...
50 ml of 0.100M solution of a weak acid HB titrated with NaOH. Calculate ph at the start, after 10.0 ml, 50.0 ml, and 60.0 ml. Ka=1.0x10^-5 [NaOH]=0.1M
A weak acid, HA, is 0.1% ionized in a 0.2 M solution. Answer the following questions:...
A weak acid, HA, is 0.1% ionized in a 0.2 M solution. Answer the following questions: a) What is the equilibrium constant (Ka) for the dissociation of this acid? b) What is the pH of the solution? c) How much ‘weaker’ in active acidity of the HA solution compared to 0.2 M HCl solution? d) How many mls of 0.1 M NaOH would be needed to neutralize completely 250 ml of the 0.2 M HA solution?
Tuo UF Weak Acid with Strong Base 5 of 7 > A certain weak acid, HA,...
Tuo UF Weak Acid with Strong Base 5 of 7 > A certain weak acid, HA, with a Ka value of 5.61 x 10 Constants Periodic Table A titration involves adding a reactant of known quantity to a solution of an another reactant while monitoring the equilibrium concentrations. This allows one to determine the concentration of the second reactant. The equation for the reaction of a generic weak acid HA with a strong base is HA(aq) + OH (aq) +...
36.53 mL of a 0.223 M solution of weak acid HA are titrated with 0.2 M...
36.53 mL of a 0.223 M solution of weak acid HA are titrated with 0.2 M NaOH. What is the pH of the solution after 8.25 mL of the NaOH have been added? The Ka for the weak acid is 0.0000077101.
33.79 mL of a 0.157 M solution of weak acid HA are titrated with 0.22 M...
33.79 mL of a 0.157 M solution of weak acid HA are titrated with 0.22 M NaOH. What is the pH of the solution after 12.98 mL of the NaOH have been added? The Ka for the weak acid is 0.0000005732.
A buffer system contains 0.225M HA (a weak acid) and 0.225M NaA (salt of the weak...
A buffer system contains 0.225M HA (a weak acid) and 0.225M NaA (salt of the weak acid). What is the pH of the buffer? (Ka for HA = 7.2 x 10-4) a. 7.2 x 10-4 b. 4.86 c. 3.14 d. -3.14 e. not enough information
1.A 1.76 M solution of a weak acid HA is found to have a pH of 2.22 Determine Kg of the acid Determine Kb of its conjugate base, A Determine [OH'] in a 2.00 M solution of the weak acid's sodium salt, NaA M Determine the pH of a 2.00 M solution of the sodium salt, NaA 2.The pH of a 1.93 M solution of a weak base B is measured to be 10.82 Determine Kp of the base Determine...
50.0 mL sample of the weak acid
the concentration of the weak acid = 0.15 M
25 mL of the week acid into 100 mL beaker
titrated this solution of 0.21 M NaOH
moles of weak acid = 3.75*10^-3
moles of NaOH = moles of week acid
c) How many milliliters of the NaOH are required to neutralize the sample of weak acid? d) How many moles of NaOH have been added at one half of the volume in part...
Tuo UF Weak Acid with Strong Base 5 of 7 > A certain weak acid, HA, with a Ka value of 5.61 x 10 Constants Periodic Table A titration involves adding a reactant of known quantity to a solution of an another reactant while monitoring the equilibrium concentrations. This allows one to determine the concentration of the second reactant. The equation for the reaction of a generic weak acid HA with a strong base is HA(aq) + OH (aq) +...
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