The pH of the solution formed by mixing 50 mL of 0.1 M NaH2PO4 and
10 mL of 0.2 M NaOH You calculate. (Ka1 = 7.5 x 10-3, Ka2 = 6.32 x
10-8, Ka3 = 4.5 x 10-13)
a)7.02 b) 5.71 c) 9.69 d) 6.28 e) anything
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The pH of the solution formed by mixing 50 mL of 0.1 M NaH2PO4 and 10...
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In the titration of 250.0 mL of 0.20 M H3PO4 with 0.10 M NaOH, the pH of the solution after the addition of some NaOH is 4.66. Which of the following phosphate-containing species is present in the largest amount? For H3PO4, Ka1 = 7.5 × 10–3, Ka2 = 6.2 × 10–8, and Ka3 = 4.8 × 10–13.
A buffer consists of 0.24 M NaH2PO4 and 0.47 M Na2HPO4. Given that the K values for H3PO4 are, Ka1 = 7.2 x 10-3, Ka2 = 6.3 x 10-8, and Ka3 = 4.2 x 10-13, calculate the pH for this buffer.
A buffer consists of 0.24 M NaH2PO4 and 0.47 M Na2HPO4. Given that the K values for H3PO4 are, Ka1 = 7.2 x 10-3, Ka2 = 6.3 x 10-8, and Ka3 = 4.2 x 10-13, calculate the pH for this buffer. I know that the answer is 7.49 because pH = -log(6.3 x 10-8) + log(0.47/0.24). What I want to know is WHY 6.3 x 10-8 was used instead of Ka1 or Ka3. Thanks.
A buffer consists of 0.34 M NaH2PO4 and 0.28 M Na2HPO4. Given that the values for H3PO4 are, Ka1 -7.2 x 10-3 Ka2 = 6.3 x 10-8 and Ka3 = 4.2x 10-13, calculate the pH for this buffer. Selected Answer: Correct Answer: [None Given] 7.12 10.02
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What is the pH of a solution obtained after mixing 20 mL of 0.1 M HI solution with 10 mL of 0.2 M HCl?
A 0.200 M solution of HCl is added to a solution containing 0.150 moles of sodium phosphate (Na3PO4). The resulting solution is then diluted to exactly 1.00 L, at which time the pH was found to be pH 8.00. What is the concentration of H2PO4- in the solution? For phosphoric acid, Ka1 = 7.11 x 10-3, Ka2 = 6.32 x 10-8, and Ka3 = 7.1 X 10-13.
What is the equilibrium pH of a 0.515 M solution of H3PO4 (aq)? (Ka1 = 7.5 × 10–3 , Ka2 = 6.2 × 10–8 , Ka3 = 4.8 × 10–13) a. 1.23 b. 3.75 c. 12.32 d. 6.30 e. 7.21