You have 250. mL of 0.125 M HCl. Using a volumetric pipet, you take 50.00 mL of that solution and dilute it to 100.00 mL in a volumetric flask. Now you take 5.00 mL of that solution, using a volumetric pipet, and dilute it to 100.00 mL in a volumetric flask. What is the concentration of hydrochloric acid in the final solution? Concentration = M

What volume in mL of an 11.6 M HCIO, (100.5 g/mol) solution is needed to make 500.0 mL of a 7.59 M HCIO4 solution? Do not put units in your answer. Report your answer as a whole number (no decimal places).

You have 559 ml of 3.29 M HCl.  Using a volumetric pipet, you take 297 ml of that solution and dilute it to 612 ml in a volumetric flask.  Now you take 100.00 ml of that solution and dilute it to 176 ml in a volumetric flask.  What is the concentration of hydrochloric acid in the final solution?

You want to determine the % of an acetic acid sample solution by acid/base titration. Therefore, you prepare a NaOH solution. To determine the exact concentration of this NaOH you titrate exactly 390.3 mg KHPhthalate (M = 204.22 g/mol) with this NaOH solution requiring 8.2 ml. Subsequently you use this NaOH solution to titrate 25.0 ml of your acetic acid sample (M(acetic acid)=60.05 g/mol, density of solution 1 g/ml) resulting in a consumption of 6.9 ml of the NaOH solution. = Please give all relevant reaction equations (with correct stoichiometry). Calculate the exact concentration (in mol/L) of the NaOH solution. Please calculate the weight-% of acetic acid in the sample solution. Which indicator would you use for this titration/at which pH range would you expect the equivalence point? (8)