1. A 25.0 mL of Ba(OH)2 of unknown concentration was placed in the Erlenmeyer flask. A titration was performed quickly to determine the concentration of nitric acid. About 45 mL of 0.062 M nitric acid was required to neutralize the barium hydroxide. Find the molarity of Ba(OH)2 The balanced equation is : Ba(OH)2 + 2HNO3 → Ba(NO3)2 + 2H2O

1. A 25.0 mL of Ba(OH)2 of unknown concentration was placed in the Erlenmeyer flask. A titration was performed quickly to determine the concentration of nitric acid. About 45 mL of 0.062 M nitric acid was required to neutralize the barium hydroxide. Find the molarity of Ba(OH)2 The balanced equation is : Ba(OH)2 + 2HNO3 → Ba(NO3)2 + 2H2O

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

You have 250. mL of 0.106 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 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?
How many grams of Cu(OH)2 will precipitate when excess KOH solution is added to 69.0 mL of 0.584 M CuCl2 solution? CuCl2(aq)+2KOH(aq) → Cu(OH)2 (s) + 2KCl(aq) g
You are making 750 mL of a 0.7 M Ca(OH)2 solution. How many moles of Ca(OH)2 will be added? How many grams of Ca(OH)2 will be massed out in a weigh boat?
Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory to standardize strong base solutions. It has the unwieldy formula of KHC3H,04. This is often written in shorthand notation as KHP. What volume of a 0.438 M sodium hydroxide solution is needed to exactly neutralize 3.48 grams of KHP ?
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?
Sodium hydroxide is used extensively in acid-base titrations because it is a strong, inexpensive base. A sodium hydroxide solution was standardized by titrating 43.00 mL of 0.1425 M standard hydrochloric acid. The initial buret reading of the sodium hydroxide was 1.07 mL, and the final reading was 38.97 mL. What was the molarity of the base solution?
A student mixes 100.0 mL of 0.500 M AgNO3 with 100.0 mL of 0.500 M CaCl2. Write the balanced molecular equation for the reaction. Write the net ionic equation for the reaction. How many grams of precipitate will form? What is the concentration of Ag+, NO3‒, Ca2+, and Cl‒ in the final solution (assume volumes are additive).
4. In the reaction of Zinc(II) carbonate and HCl forming Zinc(II) chloride, water and CO2 there was 45g Zinc(II) carbonate and it took 181mL of HCl solution to completely react. Find the molarity of the HCl solution used.
1. A student was asked to react silver nitrate with sodium during a stoichiometry lab. The student react 12.3 g of silver nitrate with 7.83 g of sodium sulfate to produce the following products. Na2SO4(aq) + 2 AgNO3 (aq) -> Ag2SO4(s) + 2 NaNO3(aq) a) predict the mass of percipitate that the student should obtain.
A student performs the titration of hydrochloric acid with sodium hydroxide. A 20.00 mL aliquot of the HCl solution required 30.50 mL of a 0.150 mol L-1 NaOH solution to reach the end point in the titration using a phenolphthalein indicator. Write the balanced molecular equation for this reaction AND determine the concentration of the original hydrochloric acid solution. Give your answer to the correct number of significant figures.
A 25.5-mL sample of a 1.68 M potassium chloride solution is mixed with 14.6 mL of a 0.870 M lead(II) nitrate solution and this precipitation reaction occurs: 2KCl(aq)+Pb(NO3)2(aq)→PbCl2(s)+2KNO3(aq) The solid PbCl2 is collected, dried, and found to have a mass of 2.47 g. Determine the limiting reactant, the theoretical yield, and the percent yield. Determine the limiting reactant. Express your answer as a chemical formula. Determine the theoretical yield. Express your answer to three significant figures.