Calculate the concentration of a sodium hydroxide solution if it takes 15.6 mL of a 0.1243 M solution of sulfurous acid to reach the endpoint of titration for a 25.00 mL sample of the sodium hydroxide solution.   2 NaOH (aq)  +   H2SO3 (aq)  →  2 H2O (l)  +   Na2SO3 (aq)

On their third titration trial, the CHM 111 student used 18.80 mL of 0.205 M NaOH(aq) to neutralize 25.0 mL of HCl(aq). Calculate the molar concentration of the HCl solution to the correct number of significant figures.

The amount of  I−3(aq)  in a solution can be determined by titration with a solution containing a known concentration of  S2O2−3(aq)  (thiosulfate ion). The determination is based on the net ionic equation 2S2O2−3(aq)+I−3(aq)⟶S4O2−6(aq)+3I−(aq) Given that it requires  33.5 mL  of  0.430 M Na2S2O3(aq)  to titrate a  15.0 mL  sample of  I−3(aq),  calculate the molarity of  I−3(aq)  in the solution.

A 25.00 mL sample of boric acid requires 32.57 mL of 0.2514 M NaOH to reach the endpoint of titration. H3BO3 (aq) + 3 NaOH (aq) → Na3BO3 (aq)   + 3 H2O (l) Determine the concentration of boric acid in the sample. Write the full and net ionic equation for the reaction.

The amount of I (aq) in a solution can be determined by titration with a solution containing a known concentration of S₂O3(aq) (thiosulfate ion). The determination is based on the net ionic equation 2S₂O3(aq) + 13(aq) · → S₂O²(aq) + 31¯ (aq) Given that it requires 27.4 mL of 0.260 M Na₂S₂O3(aq) to titrate a 10.0 mL sample of 13 (aq), calculate the molarity of I3 (aq) in the solution. [H] = M

Calculate the molar concentration HCl when 250 mL of 0.10 M HCl is mixed with 150 mL of 0.10 M NaOH in a beaker.                    HCl (aq)  + NaOH (aq)   →    NaCl (aq)   + H2O (l)

A solution of Ca(OH)2 (aq) of unknown concentration is titrated to the equivalence point with 0.250 M HCl(aq). The reading on the acid buret is 11.25 mL at the first equivalence point.  The reading on the Base buret at the equivalence point is 10.10 mL. What is the concentration (molarity) of the Ca(OH)2 solution?

A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 16.8 mL of HNO₃ was required. Write the balanced chemical equation based on the following description: solid calcium hydroxide reacts with aqueous nitric acid to produce the aqueous calcium nitrate and liquid water.  Ca(OH)2(aq)+HNO3(aq)------

If 28.0 g of NaOH is added to 0.600 L of 1.00 M Mn(NO₃)₂, how many grams of Mn(OH)₂ will be formed in the following precipitation reaction? 2 NaOH(aq) + Mn(NO₃)₂(aq) → Mn(OH)₂ (s) + 2 NaNO₃(aq)

A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. 1. If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) 2.The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. 3. Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.