Homework Answers
9) pOH = 1/2(pKb - logC)
= 1/2(4.74-log(0.1)]
=> 2.87
pH = 14-2.87 => 11.13
B) pH for salt
pH = 1/2(14-pKb-logC)
= 1/2(14-4.74-log(0.10)]
= 5.13
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4-l0.2 Solution 8 10.0 mL of solution 5 + find the limiting reager Calculated pH h...
Solution pH Table 4. Theoretical pH of strong acids and bases and weak acids and hases...
Solution pH Table 4. Theoretical pH of strong acids and bases and weak acids and hases Solution difference Theoretical Theoretical Theoretical pH from Measured Theoretical pH from Measured Strong Acid Strong Base Strong Acid Weak Acid Weak Base Weak Acid 0.10 M 0.010 M 0.0010 M 0.00010 M 2. Kor Ks can also be calculated from the pH. See Example 2. in the discussion under weak acids and bases. Calculate Kfrom your measured pH of the 0.10 M solution of...
Please walk me step by step on how to get the calculated pH for the weak...
Please walk me step by step on how to get the calculated pH
for the weak acid. I dont understand this at all and really need
step by step not just a brief explanation. Thank you
A pH of Acid Solutions: 1. Strong Acid Measured pH [HCI), 1.48 0.10M [HCI), 2.17 0.010M Molarity (0.0 (1.0) -M2 (10.00 Calculated pH 1.00 2.00 10o = 0.01 -log(0.01)=2 [HC,H,O, Kas 1.8x10s Weak Acid Measured pH [HC,H,O, 3.44 0.01M Molarity 0.10M Calculated pH Compare...
1) Find the Difference between measured pH and calculated theoretical pH of solutions 1-6 for [HC2H3O2]...
1) Find the Difference between measured pH and calculated
theoretical pH of solutions 1-6 for
[HC2H3O2] (M) and
[C2H3O2−] (M)
2) Find the Difference between measured pH and calculated
theoretical pH of solutions 1-6.
3) In this experiment, we define the buffer capacity of a buffer
as the number of drops of either 3.0 M HCl or 3.0 M NaOH needed
before the pH of the solution changes by more than 0.5 pH units.
For example, if the pH of...
Part 1 (a) Calculate the pH at 25°C of a 0.10 M solution of a weak...
Part 1 (a) Calculate the pH at 25°C of a 0.10 M solution of a weak base with a Kb of 2.6 ×10−11 Part 2 (a) Calculate the pH for each of the following solutions at 25°C. (b) 0.12 M NH3 (Kb for NH3 = 1.8 ×10−5) (c) 0.050 M C5H5N (pyridine). (Kb for pyridine = 1.7 × 10−9)
QUESTION 4 What is the pH of 31.56 mL of a 0.1528 M solution of a...
QUESTION 4 What is the pH of 31.56 mL of a 0.1528 M solution of a weak monoprotic basic base (B:, Kb = 2.41 x 10-0) @ the midway point of a titration with 0.1236 M HCIO3? %3D Your answer must have 2 decimal places. QUESTION 5 What is the pH of 37.88 mL of a 0.1142 M solution of a weak basic base (B:, Kp = 7.95 x 10-4) that has been titrated with 18.45 mL of 0.1831 M...
How do you find the degree of ionization of the solutions when accounting for the dillution...
How do you find the degree of ionization of the solutions when
accounting for the dillution effect of adding 10 mL of water? Also
for the second page, how do you calculate pH with a buffer using
the Henderson-Hasselbalch equation?
Solution 2 - 10.0 mL of 0.1 M HC2H302 +10.0 mL H20 Measured pH_2.42 To determine the [H3O+], account for the dilution effect of adding 10.0 mL of water, and use MV1 = M2V2 Degree of lonization of solution 2...
Can anyone please help with how to calculate degree of ionization for the first 3 solutions...
Can anyone please help with how to calculate degree of
ionization for the first 3 solutions as well as how to calculate
the expected pH for solution 4? thank you!
Experiment 8: Equilibria of Weak Acids and Bases Lab Report Sheet 1 Composition 20.0 mL of 0.1 M HC2H302 - (A weak acid) pH 12.76 2.42 2.59 10.0 mL of 0.10 M HC2H3O2 + 10.0 mL H20 - (effect of dilution on the degree of ionization of weak acid) 10.0...
3) Kb for NH3 1.8 x 10-5 a) Calculate the pH of a buffer solution that...
3) Kb for NH3 1.8 x 10-5 a) Calculate the pH of a buffer solution that is 0.100 M NH3 and 0.120 M NHANO3. b) What is the pH after 60.0 mL of 0.010 M HCl is added to 90.0 mL of the buffer solution in 2(a). Assume the change in volume is additive. c) What is the pH after 60.0 mL of 0.010 M Ca(OH)2 is added to 90.0 mL of the buffer solution in 2(a). Assume the change...
how would you calculate the expected pH for solution 7, 8, 9, 10, and 11? (I...
how
would you calculate the expected pH for solution 7, 8, 9, 10, and
11? (I am confused on how you calculate the dilutions for finding
the expected pH too)
Ka= 1.4x10^-5
pKa= 4.85
Part B - The Effect of Adding Acid or Base to a Buffered Solution Solution 6 16. Prepare a buffer solution by mixing 30.0 mL of 0.10 M HOAc and 40.0 mL of 0.10 M NaOAc. Measure the pH of the resulting solution with the pH...
1. Calculate the equilibrium concentrations of all species present and the pH of a solution obtained...
1. Calculate the equilibrium concentrations of all species present and the pH of a solution obtained by adding 0.100 moles of solid NaOH to 1.00 L of 15.0 M NH3. Kb = 1.8 × 10–5 2. One mole of a weak acid HA was dissolved in 2.0 L of water. After the system had come to equilibrium, the concentration of HA was found to be 0.45 M. Calculate the Ka for this weak acid. 3. Calculate the pH of a...
Solution pH Table 4. Theoretical pH of strong acids and bases and weak acids and hases Solution difference Theoretical Theoretical Theoretical pH from Measured Theoretical pH from Measured Strong Acid Strong Base Strong Acid Weak Acid Weak Base Weak Acid 0.10 M 0.010 M 0.0010 M 0.00010 M 2. Kor Ks can also be calculated from the pH. See Example 2. in the discussion under weak acids and bases. Calculate Kfrom your measured pH of the 0.10 M solution of...
Please walk me step by step on how to get the calculated pH
for the weak acid. I dont understand this at all and really need
step by step not just a brief explanation. Thank you
A pH of Acid Solutions: 1. Strong Acid Measured pH [HCI), 1.48 0.10M [HCI), 2.17 0.010M Molarity (0.0 (1.0) -M2 (10.00 Calculated pH 1.00 2.00 10o = 0.01 -log(0.01)=2 [HC,H,O, Kas 1.8x10s Weak Acid Measured pH [HC,H,O, 3.44 0.01M Molarity 0.10M Calculated pH Compare...
1) Find the Difference between measured pH and calculated
theoretical pH of solutions 1-6 for
[HC2H3O2] (M) and
[C2H3O2−] (M)
2) Find the Difference between measured pH and calculated
theoretical pH of solutions 1-6.
3) In this experiment, we define the buffer capacity of a buffer
as the number of drops of either 3.0 M HCl or 3.0 M NaOH needed
before the pH of the solution changes by more than 0.5 pH units.
For example, if the pH of...
QUESTION 4 What is the pH of 31.56 mL of a 0.1528 M solution of a weak monoprotic basic base (B:, Kb = 2.41 x 10-0) @ the midway point of a titration with 0.1236 M HCIO3? %3D Your answer must have 2 decimal places. QUESTION 5 What is the pH of 37.88 mL of a 0.1142 M solution of a weak basic base (B:, Kp = 7.95 x 10-4) that has been titrated with 18.45 mL of 0.1831 M...
How do you find the degree of ionization of the solutions when
accounting for the dillution effect of adding 10 mL of water? Also
for the second page, how do you calculate pH with a buffer using
the Henderson-Hasselbalch equation?
Solution 2 - 10.0 mL of 0.1 M HC2H302 +10.0 mL H20 Measured pH_2.42 To determine the [H3O+], account for the dilution effect of adding 10.0 mL of water, and use MV1 = M2V2 Degree of lonization of solution 2...
Can anyone please help with how to calculate degree of
ionization for the first 3 solutions as well as how to calculate
the expected pH for solution 4? thank you!
Experiment 8: Equilibria of Weak Acids and Bases Lab Report Sheet 1 Composition 20.0 mL of 0.1 M HC2H302 - (A weak acid) pH 12.76 2.42 2.59 10.0 mL of 0.10 M HC2H3O2 + 10.0 mL H20 - (effect of dilution on the degree of ionization of weak acid) 10.0...
3) Kb for NH3 1.8 x 10-5 a) Calculate the pH of a buffer solution that is 0.100 M NH3 and 0.120 M NHANO3. b) What is the pH after 60.0 mL of 0.010 M HCl is added to 90.0 mL of the buffer solution in 2(a). Assume the change in volume is additive. c) What is the pH after 60.0 mL of 0.010 M Ca(OH)2 is added to 90.0 mL of the buffer solution in 2(a). Assume the change...
how
would you calculate the expected pH for solution 7, 8, 9, 10, and
11? (I am confused on how you calculate the dilutions for finding
the expected pH too)
Ka= 1.4x10^-5
pKa= 4.85
Part B - The Effect of Adding Acid or Base to a Buffered Solution Solution 6 16. Prepare a buffer solution by mixing 30.0 mL of 0.10 M HOAc and 40.0 mL of 0.10 M NaOAc. Measure the pH of the resulting solution with the pH...
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