You are standardizing a solution of KOH. You weigh out 2.34 g of potassium hydrogen phthalate, dissolve it in water and add 2 drops of phenolphthalein solution. You fill the buret with the KOH solution to an initial reading of 2.33mL. You add the KOH solution to the flask and when the endpoint is reached you record the final buret reading to be 34.11mL. Calculate the molarity of KOH in the solution.

You are standardizing a solution of KOH. You weigh out 2.34 g of potassium hydrogen phthalate, dissolve it in water and add 2 drops of phenolphthalein solution. You fill the buret with the KOH solution to an initial reading of 2.33mL. You add the KOH solution to the flask and when the endpoint is reached you record the final buret reading to be 34.11mL. Calculate the molarity of KOH in the solution.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

5.00 g of solid Al(NO3)3 was added to enough water to make a solution with a total volume of 100.0 mL. Al(NO3)3 is very soluble in water and this much solid will fully dissolve in a 100.0 mL solution. If 65 mL of water was added to the original 100.0 mL Al(NO3)3 solution described to the left in order to dilute the solution. Calculate the new diluted solution concentration, in Molarity? Assume the volumes of the 2 solutions are additive.
Titration of a 11.0 mLmL solution of HClHCl requires 32.4 mLmL of 0.11 MM NaOHNaOH. What is the molarity of the HClHCl solution? Express your answer using two significant figures.
How many grams of NaCl are required to precipitate most of the Ag* ions from 2.50 × 10² mL of 0.0147 M AgNO3 solution? Round your answer to 3 significant digits. g NaCl x10 X 5
If 50.1 mL of 0.128 M hydrochloric acid requires 17.5 mL of NaOH solution to reach the endpoint, what is the molarity of the NaOH solution? Include three decimal places in your answer.
A 500.0-mL solution was prepared by dissolving 25.00 mL of methanol (CH3OH, density 5 0.791 4 g/mL) in chloroform. Find the molarity of the methanol.
Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits.
What mass of cobalt III hydroxide, Co(OH)3 is needed to make 1.2 liters of a 0.21 M cobalt III hydroxide solution? What volume of barium chloride, BaCl2 is needed to make a 2.5 M barium chloride solution with 0.25 mol BaCl2? Calculate the molarity of 14.2 grams of sugar, C12H22O11 in 1,500. mL of solution. How many grams of potassium nitrate, KNO3 are required to prepare 1.50 L of a 2.80M solution? A solution is prepared by mixing 200.0 g of water, H2O, and 200.0 g of ethanol, C2H5OH. Determine the mole fractions of each substance. Calculate the molality of 15.0 grams of KBr dissolved in 750.0 mL pure water. What mass of ammonium sulfate, (NH4)2SO4 must be added to prepare 400.0 g of a 7.0% solution of ammonium sulfate in water?
You are standardizing a NaOH solution and find that it requires 21.71mL of NaOH to neutralize 1.589g of KHP (molar mass 204.22 g/mol). What is the NaOH concentration in M (mol/L)?
If 49.7 mL of 0.11 M hydrochloric acid requires 14.3 mL of NaOH solution to reach the endpoint, what is the molarity of the NaOH solution? Include three decimal places in your answer.
An analytical chemist weighs out 0.091 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1200M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 23.2 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 2 significant digits. mol ?
A chemistry student is given 1.00 L of a clear aqueous solution at 17 degrees Celsius. He is told an unknown amount of a certain compound X is dissolved in the solution. The student allows the solution to cool to 17 degrees Celsius. The solution remains clear. He then evaporates all of the water under vacuum. A precipitate remains. The student washes, dries and weighs the precipitate. It weighs 0.12 kg. Using only the information above, can you calculate the solubility of X in water at 17° C? If you said yes, calculate it and be sure your answer has a unit symbol and 2 significant digits.
mL When blood is donated, sodium oxalate solution is used to precipitate Ca2+, which triggers clotting. A 122.0-mL sample of blood contains 9.70 × 10-5 g Ca A technologist treats the sample with 100.0 mL of 0.1550 M Na₂C₂O. Calculate [Ca2+] after the treatment. Be sure your answer has the correct number of significant figures. Note: Reference the Solubility product constants (Ksp) table for additional information. M Ca2+ 5