You have 250. mL of 0.208 M HCl . Using a volumetric pipet, you take 25.00 mL of that solution and dilute it to 100.00 mL in a volumetric flask. Now you take 10.00 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?

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)

1. If 10. g of AgNO3 is available, what volume of 0.40 M AgNO3 solution can be prepared? Volume =   mL? 2. A 7.52-g sample of a diprotic acid requires 179.0 mL of a 0.750 M NaOH solution for complete neutralization. Determine the molar mass of the acid.  g/mol?

An analytical chemist weighs out 0.065 of an unknown monoprotic acid into a 250mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 6.4mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 2

The iodine contained in every one mL of the 0.010 M iodine solution in the buret will react with 1.76 mg of vitamin C. (In other words, every mL of iodine solution needed for the titration indicates the presence of 1.76 mg of vitamin C in the juice sample.) If your titration used 5.86 mL of iodine solution, what mass of vitamin C is in your fruit juice sample (in milligrams, mg)?

You wish to make a 0.350 M hydroiodic acid solution from a stock solution of 6.00 M hydroiodic acid. How much concentrated acid must you add to obtain a total volume of 75.0 mL of the dilute solution? ___mL

A student is asked to standardize a solution of calcium hydroxide. He weighs out 0.945 g potassium hydrogen phthalate (KHC8H404, treat this as a monoprotic acid). It requires 27.4 mL of calcium hydroxide to reach the endpoint. A. What is the molarity of the calcium hydroxide solution? M This calcium hydroxide solution is then used to titrate an unknown solution of hydrochloric acid. B. If 12.3 mL of the calcium hydroxide solution is required to neutralize 29.7 mL of hydrochloric acid, what is the molarity of the hydrochloric acid solution? M

A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1840 M standard sodium hydroxide solution. He takes a 25.00 mL sample of the original acid solution and dilutes it to 250.0 mL. Then, he takes a 10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 13.34 mL of the standard solution. What is the concentration of the original sulfuric acid solution? concentration: M

4

Help