50.0 mL of 0.10 M HNO2 is being titrated with 0.20 M NaOH.
What is the pH after 25.0 mL NaOH has been added?
What is the pH after 35.0 mL NaOH has been added?
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50.0 mL of 0.10 M HNO2 is being titrated with 0.20 M NaOH. What is the...
6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added, the pH of the resulting solution was 6.70. After 50.0 mL of NaOH was added, the pH of the solution was 8.00. What are the values of Ka1 and Ka2? 6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added,...
50.0 mL of 0.090 M nitrous acid (HNO2, Ka = 7.1 x 10-4), is titrated with 0.100 M NaOH, requiring 45.0 mL of strong base to reach the equivalence point. (a) What will be the pH after 35.0 mL of NaOH have been added? (b) What will be the pH at the equivalence point? (c) What will be the pH after 60.0 mL of NaOH have been added?
A 25.0 ml sample of 0.20 M Formic Acid (HCO2H, aq) is titrated with 0.10 M KOH(aq). What is the pH after 50.0 mL of the 0.10 M KOH has been added?
1. A solution (50.0 mL) of 0.125 M HCl is being titrated with 0.125 M KOH. What species are present in this solution, and what is the pH: (a) Before any KOH solution has been added? (b) After 50.0 mL KOH solution has been added? (c) After 25.0 mL KOH has been added? (d) After 75.0 mL KOH has been added?
1. A solution (50.0 mL) of 0.125 MHCI is being titrated with 0.125 M KOH. What species are present in this solution, and what is the pH: (a) Before any KOH solution has been added? (b) After 50.0 mL KOH solution has been added? (c) After 25.0 mL KOH has been added? (d) After 75.0 mL. KOH has been added
25 mL of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH after 30 ml of NaOH have been added? Ka for acetic acid = 1.8 x 10^-5.
50.0 mL of 0.275 M HNO2 is titrated to its equivalence point with 1.00 M NaOH. What is the pH at the equivalence point? Ka for HNO2 is 4.0x10^-4
50.0 mL of 0.150 M HNO2 is titrated to its equivalence point with 1.00 M NaOH. What is the pH at the equivalence point?
1. A solution (50.0 mL) of 0.125 M HCl is being titrated with 0.125 M KOH. What species are present in this solution, and what is the pH: (a) Before any KOH solution has been added? (b) After 50.0 mL KOH solution has been added? (c) After 25.0 mL KOH has been added? (d) After 75.0 mL KOH has been added? Can all work be shown? Equations/ Ice charts If applicable-please include them. I need to understand. Thank-you in advance.
A 50.0 mL sample of 0.11 M nitrous acid is titrated with 0.22 M NaOH. Calculate the pH to one decimal place when the following volumes of NaOH have been added. 0.00 mL 22.0 mL 25.0 mL 33.0 mL