Ka = 1.3*10^-5
pKa = - log (Ka)
= - log(1.3*10^-5)
= 4.886
use:
pH = pKa + log {[conjugate base]/[acid]}
= 4.886+ log {0.8/0.45}
= 5.136
Answer: 5.14
What is the pH for a buffer that consists of 0.45 M CH3CH2COOH and 0.80 M...
What is the pH of a buffer that consists of 0.45 M CH3COOH and 0.35 M CH3COONa? Ka = 1.8 x 10-5 So the answer is 4.64. However, I was under the impression that it is Ka * (base/acid). So wouldn't that be 1.8 x 10^-5 * (.35/.45)? Isn't the CH3COONa the base? Someone please explain. Thank you.
What is the pH of a buffer that consists of 0.85 M CH3COOH and 0.35 M CH3COONa? Ka = 1.8 × 10–5 Select one: A. 4.64 B. 4.31 C. 5.52 D. 5.00 E. 4.85
What is the pH of a buffer that consists of 0.15 M CH3CH2COOH and 0.20 M CH3CH2COONa? What is the pH of this buffer after the addition of 5.0 mL of 0.10 M NaOH to 1.0 L of the solution?
QUESTION 6 What is the buffer component ratio, (CH3CH2COO(CH3CH2COOH) of a propanoate buffer that has a pH of 4.77. Ka of CH3CH2COOH is 1.3 x 10-5. Enter your answer with three decimal places and no units.
3. (a) Calculate the pH of a solution 0.145 M with respect to CH3CH2COOH and 0.115 M with respect to K+CH3CH2COO-. Ka = 1.3 x 10 – 5 ; pKa = 4.89 (b) Calculate the pH of the same solution after adding 0.015 M KOH. (c) Calculate the pH of the same solution as in part (a) but after addition of 0.015 M HBr.
A student prepares a buffer by adding 200.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH3CH2COOH. What is the pH of this buffer? Ka = 1.3 × 10–5
Top question. P1. (Sec. 16.2) What is the pH of a solution prepared by adding 0.45 moles of formic acid HCO2H, and 0.40 moles of sodium formate, NaCO,H, in enough water to make a 1.0-liter solution? (Formic Acid: K 1.81 10-) a) 4.32 b) 3.69 c) 5.52 d) 7.32 e) 9.11 P2. (Sec. 16.2) What is the pH of a solution prepared by adding 100 mL of a 0.25 M solution of sodium acetate, NaC2H,O2, into 110 mL of 0.30...
A buffer of pH 9.24 is to be prepared from a weak acid and its salt. The best acid from which to prepare the buffer is (a) phthalic acid, K1 = 1.3 x 10-3 (1st ionization) (b) hydrohen phthalate, K2 = 3.9 x 10-5 (c) arsenious acid, Ka = 6 x 10-10 (d) formic acid, Ka = 1.8 x 10-5 (e) phenol, Ka = 1.3 x 10-10 Please explain all options.
Consider two buffer solutions. Buffer 1 consists of 0.50 M HA and 0.25 M KA, and Buffer 2 is made from 0.050 M HA and 0.050 M NaA. How do the pHs of these buffer solutions compare? Select one or more: a. The pH of Buffer 1 is twice the pH of Buffer 2. b. The pH of Buffer 1 is half the pH of Buffer 2. c. The pH of Buffer 1 is equal to the pH of Buffer...
A 10.0 mL sample of 0.75 M CH3CH2COOH(aq) is titrated with 18.0 mL of 0.30 M NaOH(aq) (adding NaOH to CH3CH2COOH). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture. Ka of CH3CH2COOH is 1.3 \times × 10−5. Henderson–Hasselbalch equation: LaTeX: pH=pK_a+\log\frac{\left[base\right]}{\left[acid\right]} p H = p K a + log [ b a s e ] [ a c i d ] 2046 HW10 Q1-1.jpg 1) After adding the NaOH...