Calculate the pH when 40.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)
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Calculate the pH when 40.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO...
Calculate the pH when 10.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 x 10-9)
Submit Question 12 of 30 Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 16.0 mL of 0.300 M HBrO (Ka = 2.5 x 10) 8. 1 3 N 4 5 6 с 7 8 9 +/- 0 X 100
calculate the pH & POH of a mixture containing 20.0 mL of 0.150 m HBr mixed W/ 40.0 mL of water.
Quest. 7 (30 pts). Benzoic acid (C6H5COOH), 40.0 mL of 0.150 M, is being titrated with 0.300 M potassium hydroxide (KOH). Calculate the pH a) before any addition of base, b) at the half neutralization (half equivalent) point, and c) at the equivalent point. The Ka of C6H5COOH is 6.5 x 10-5. Use the appropriate tables when necessary.
A 50.0 mL solution of 0.150 M KOH is titrated with 0.300 M HCl. Calculate the pH of the solution after the addition of the following amounts of HCl. d) 18.0 mL HCl e) 24.0 mL HCl g) 26.0 mL HCl h) 29.0 mL HCl
Calculate the pH of the resulting solution if 30.0 mL of 0.300 M HCl(aq) is added to (a) 40.0 mL of 0.300 M NaOH(aq). Number pH= 12.63 (b) 20.0 mL of 0.400 M NaOH(aq). Number pH= 1.22
Calculate the pH for each case in the titration of 50.0 mL of 0.150 M HClO(aq) with 0.150 M KOH(aq). Use the ionization constant for HClO.What is the pH before addition of any KOH?pH=What is the pH after addition of 25.0 mL KOH?pH=What is the pH after addition of 40.0 mL KOH?pH=What is the pH after addition of 50.0 mL KOH?pH=What is the pH after addition of 60.0 mL KOH?pH=No referals please since the one I got with altered number did not work.
Consider the titration of a 40.0 mL sample of 0.150 M HCl with 0.200 M KOH a) What is the initial pH? b) What is the pH after the addition of 10.0 mL of the KOH? c) What is the pH at the equivalence point? d) What is the pH after 40.0 mL of KOH has been added?
A 40.0 mL sample of 0.150 M HNO2 (Ka = 4.60 x 10-4) is titrated with 0.200 M KOH. Calculate: a. the pH after adding 10.00 mL of KOH b. the pH at one-half the equivalence point c. the pH after adding 20.00 mL of KOH d. the volume required to reach the equivalence point e. the pH at the equivalence point f. the pH after adding 45.00 mL of KOH
Calculate the pH of a solution after 40.0 mL of 0.150 M NaOH has been added to 50.0 mL of 0.250 M HF. Ka for HF = 6.6 x 10-4 a. 12.00 b. 7.56 C. 4.74 d. 3.15 O e. 1.12