What is the pH of a solution of a strong acid with a concentration of 0.007 M?
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What is the pH of a solution of a strong acid with a concentration of 0.007...
what is the ph of a solution of a strong acid with a concentration .007 M
16. A 1.00 L solution of strong acid with a pH of 5.00 is added to a 1.00 L solution of a strong acid with a pH of 4.00. What is the final pH of the mixture? A) 4.00 D) 3.96 B) 5.00 E) 4.26 C) 4.50
16. A 1.00 L solution of strong acid with a pH of 5.00 is added to a 1.00 L solution of a strong acid with a pH of 4.00. What is the final...
What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl? Ka = 3.0 × 10-8 for HOCl. A. A) 0.30 B. B) 2.18 C. C) 6.76 D. D) 4.03 E. E)7.01 F. F) 8.92 G. G) none of these
Explain why a weak acid solution has a higher pH than a strong acid solution concentration. of the same Explain why the equivalence point of a weak acid titrated with a strong base occurs at a basic pH.
Strong Acids and [H'] (and pH) The pH of a strong acid is the concentration of the strong acid. 1.OM HCI makes 1.OM H. Except H2SO4. Its pH is a little lower than that because: H2SO4(aq) H+ (aq) + HS07 (aq) Strong acids generally have K.>>1. We assume K = . The HSO, is a weak acid: HSO2 (aq) + H+ (aq) + S0 - Ka = 1.2 * 10-2 Weak Acids and [H+] (and pH) These are weak electrolytes....
What concentration of HCl will have a pH of 5.0? b) What concentration of acetic acid will have a pH of 5.0? (For acetic acid, pKa=4.76) c) What concentration of phosphoric acid will have a pH of 5.0? (For H3PO4, pKa1 = 2.12, pKa2 = 7.21, pKa3 =12.32) d) What is the pH of a 10 mM solution of phosphoric acid? e) How much 1.0 M NaOH must be added to 100 ml of 10 mM H3PO4 to raise the...
Calculate the pH of a strong acid solution formed by mixing 83.3 mL of 0.0297 M HBrO4 with 77.2 mL of 0.129 M HNO3. a) The pH of this solution is 0.8. b) The pH of this solution is 1.1. c) The pH of this solution is 0.5. d) The pH of this solution is 4.4. e) The pH of this solution is 1.9.
The pH of a solution of a strong monoprotic acid is lower than the pH of an equal concentration of a weak monoprotic acid, yet equal volumes of both require the same volume of basic titrant to reach the equivalence point. Explain why.
a What is the pH of a solution that has a formic acid concentration of 0.020 M and a sodium formate concentration of 0.060 M? pH =
A 250.0 mL solution of a strong acid is found to have a pH of 0.54. What is the labeled (initial) concentration of this acid?