The expected endpoint when 10.00 mL of ~0.014 M KIO3 is titrated with 0.08 M S2O32- will be?
The expected endpoint when 10.00 mL of ~0.014 M KIO3 is titrated with 0.08 M S2O32-...
A 10.00 ml sample of .0.0100 M KIO3 was titrated against a solution of sodium thiosulfate to standardize it. The initial buret volume reading was 0.07 ml. The final buret reading was 6.54 ml. Calculate the [Na2S2O3].
Calculate the pH at the titration endpoint, when 35.00 mL of 0.150 M dimethylamine is titrated by 0.170 M hydrochloric acid. Please show all work
100 mL of solution containing Cl-is titrated to the endpoint with 10 mL of 0.050 M AgNO3. What was the concentration of Cl-in the sample? (the answer is 5.0x10^-3 M bt why???)
1. A 10.00 mL aliquot of 0.010 M CaCO3 is titrated with 18.22 mL of EDTA solution. What is the EDTA molarity? 2. A 250.0 mL water sample requires 30.85 mL of the EDTA solution from question 1 to reach the calmagite endpoint. What was the molarity of the hard metal ions in the water sample? 3. If the metal ions in the water sample of question 2 are assumed to be Ca2+ from CaCO3, express the concentration in ppm...
When 10.00 mL of 0.240 M HX (Ka = 4.31
10-5)
is titrated with 0.120 M KOH, the pH will increase. Calculate the
pH of the solution at each point in the titration. The
pKw is 14.000 at this temperature.
Volume of KOH (mL)
pH
0.00
2.00
4.00
6.00
8.00
10.00
12.00
14.00
16.00
18.00
20.00
22.00
24.00
26.00
28.00
5.0 ml of a solution of Ca(OH)2 is titrated with 0.033 M HCl. The endpoint is reached when 7.67 ml of HCl is dispensed. What is the concentration of OH- ions in the Ca(OH)2 solution? No units are required. Round answer to 3 decimal places.
5.0 ml of a solution of Ca(OH)2 is titrated with 0.03 M HCl. The endpoint is reached when 6.45 ml of HCl is dispensed. What is the concentration of OH- ions in the Ca(OH)2 solution? No units are required. Round answer to 3 decimal places.
When 10.00 mL of 0.240 M HX (Ka = 2.29 x 10') is titrated with 0.120 M KOH, the pH will increase. Calculate the pH of the solution at each point in the titration. The pkw is 14.000 at this temperature. pH Volume of KOH (mL) 0.00 2.00 4.00 6.00 8.00 10.00 12.00 14.00 16.00 18.00 20.00 22.00 24.00 26.00 28.00
A 25.00 mL sample of NaOH was titrated with a 0.743 M H2sO, solution. The endpoint of the titration was observed after the addition of 5.00 ml. of H2SO4. Calculate the concentration of the NaOH 2. solution.
5. A solution of hydrofluoric acid (0.27 M, 10.00 mL) was titrated with 15.0 mL of 0.13 M sodium hydroxide (K, of hydrofluoric acid = 7.20x104). Calculate the resulting pH of this solution.