By titration, it is found that 51.5 mL51.5 mL of 0.143 M NaOH(aq)0.143 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq).HCl(aq). Calculate the concentration of the HClHCl solution. [HCl]=[HCl]=

In a titration, 20.0 g of oxalic acid dihydrate was dissolved in a flask and neutralized with 31.2 mL of NaOH. Determine the molarity of the NaOH. 2NaOH(aq) + H2C2O4 ⋅ 2H2O(s) --> Na2C2O4(aq) + 4H2O(l)

The end point in a titration of 50.00 mL of aqueous NaOH was reached by the addition of 35.23 mL of 0.250 M aqueous HCI titrant. Calculate the molarity of the NaOH solution. The titration reaction equation is: NaOH(aq) + HCI (aq) —> NaCl(aq) + H2O(l)

Calculate the molarity of the HCI solution.

The flask contains 10.0 mL10.0 mL of HClHCl and a few drops of phenolphthalein indicator. The buret contains 0.110 M NaOH.0.110 M NaOH. It requires 31.4 mL31.4 mL of the NaOHNaOH solution to reach the end point of the titration. What is the initial concentration of HClHCl?

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.   A.) 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!)   B.) 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.   C.) 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.

By titration, it is found that 55.5 mL of 0.116 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution. [HCI] M

By titration it is found that 35.7 mL of 0.101 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.

ion The following table shows data from the titration of four 25.0 mL samples of a perchloric acid solution, HCIO4(aq), using a 0.225 mol/L sodium hydroxide standard solution. Bromothymol blue is used as an indicator to detect when the endpoint is reached. Titration of 25.0 mL of HCIO4 with 0.225 mol/L NaOH(aq) final burette reading (mL) initial burette reading (mL) volume of NaOH(aq) added (mL) colour at endpoint Trial 1 Use the data in the table below to answer the next two questions. Trial 2 Trial 3 Trial 4 Trial mL . . . mL mL 1 mL 19.9 0.4 2 Using the chart above, provide the volume of NaOH added for each of the trials. 38.8 3 19.3 19.9 0.2 4 38.4 19.3 blue green green green DELL

Calculate the number of grams of AgCl will precipitate out of solution if 125 mL of 0.500 M AgNO3 is combined with 275 mL of 0.235 M NaCl according to the following         AgNO3 (aq)   +    NaCl (aq)  -->  AgCl (s)   +  NaNO3 (aq)