42.04 mL of a solution of the acid HNO3 is titrated, and 52.40 mL of 0.5500-M NaOH is required to reach the equivalence point. Calculate the original concentration of the acid solution.
HNO3 + NaOH ----------> NaNO3 + H2O
millimoles of NaOH = 52.40 x 0.5500 = 28.82
28.82 millimoles HNO3 must be reacted
28.82 = 42.04 x M
M = 0.6855 M
[HNO3] = 0.6855 M
42.04 mL of a solution of the acid HNO3 is titrated, and 52.40 mL of 0.5500-M...
32.65 mL of a solution of the acid H2C2O4 is titrated, and 43.90 mL of 0.7300-M NaOH is required to reach the equivalence point. Calculate the original concentration of the acid solution.
26.24 mL of a solution of the acid H2C2O4 is titrated, and 84.20 mL of 0.4200-M NaOH is required to reach the equivalence point. Calculate the original concentration of the acid solution. How many M?
A volume of 60.0 mL of a 0.900 M HNO3 solution is titrated with 0.820 M KOH Calculate the volume of KOH required to reach the equivalence point.
A volume of 100 mL of a 0.590 M HNO3 solution is titrated with 0.660 M KOH. Calculate the volume of KOH required to reach the equivalence point.
A volume of 91.5 mL of a 0.205 M HNO3 solution is titrated with 0.196 M KOH. Calculate the volume of KOH required to reach the equivalence point. Enter in units of ml and to 2 decimal places.
A volume of 46 mL of a 0.614 M HNO3 solution is titrated with 0.431 M KOH. Calculate the volume of KOH required to reach the equivalence point. Enter in units of ml and to 2 decimal places.
A 25.0 mL NaOH solution of unknown concentration was titrated with a 0.189 M HCl solution. 19.6 mL HCl was required to reach equivalence point. In a separate titration, a 10.0 mL H3PO4 solution was titrated with the same NaOH solution. This time, 34.9 mL NaOH was required to reach the equivalence point. What is the concentration of the H3PO4 solution?
1) A solution of a weak monoprotic acid of unknown concentration was titrated with 0.23 M NaOH. If a 100.-mL sample of the acid solution required exactly 10. mL of the NaOH solution to reach the equivalence point, what was the original concentration of the weak acid? 2) During the titration on problem (2B), after 5.0 mL of NaOH addition, the pH = 3.68. What is the Ka of the weak acid? please show steps i have an exam tomorrow
17.04 ml of hydrochloric acid solution of unknown concentration is titrated with a 0.201 M standard solution of NaOH(aq). Compute the concentration of the hydrochloric acid solution given that 9.32 ml of the standard solution were added to reach the equivalence point.
A volume of 90.0 mL of a 0.750 M HNO3 solution is titrated with 0.730 M KOH. Calculate the volume of KOH required to reach the equivalence point. Express your answer to three significant figures and include the appropriate units.