A 25.00 mLmL sample of an H2SO4H2SO4 solution of unknown concentration is titrated with a 0.1372 MM KOHKOH solution. A volume of 40.22 mLmL of KOHKOH was required to reach the equivalence point

In an alkalinity titration of a 100.0 mL sample of water from a hot spring, 2.56 mL of a 0.0365 M  solution of HCl is needed to reach the first equivalence point (pH = 8.3) and another 10.42 mL is needed to reach the second equivalence point (pH = 4.0). If the alkalinity of the spring water is due only to the presence of carbonate and bicarbonate, what are the concentrations of each of them? What is the concentration of carbonate?     M        What is the concentration of bicarbonate?

In a titration of 68.0 mL of a 0.750 M solution of a triprotic acid H₃C₆H₅O₇ (citric acid) with 0.500 M NaOH, how many mL of base are required to reach the third equivalence point?

A titration of 3.36 g of an acid requires 43.72mL of 0.100M NaOH to reach the equivalence point.  What is the molar mass of the acid?

A 30.00 mL sample of 0.400 M HNO3 is titrated with 0.600 M KOH. What is the balanced neutralization chemical reaction? What volume of base (in mL) must be added to reach the equivalence point? Is the pH of the equivalence point acidic, basic, or neutral?

Calculate the pH of the buffer system made up of 0.15 M NH3NH3/0.35 M NH4ClNH4Cl.

120. A diprotic acid with a molar mass of 118.04 g/mol was titrated with 1.023 M NaOH. The equivalence point of the titration occurred at 22.16 mL. Calculate the mass of the acid.

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30.23 mL of a solution of the acid H2SO4 is titrated, and 47.20 mL of 0.8600-M NaOH is required to reach the equivalence point. Calculate the original concentration of the acid solution.

A titration of 40.0 mL of a sulfuric acid (H₂SO₄) solution of unknown concentration with a standardized 1.55 M Ba(OH)₂ solution requires 23.0 mL to reach the second equivalence point. What is the concentration of the H₂SO₄ solution?