You have a mixture of oxalic acid, H₂C2O4, and another solid that does not react with sodium hydroxide. If 25.52 mL of 0.580 M NaOH is required to titrate the oxalic acid in the 4.207 g sample to the second equivalence point, what is the mass percent of oxalic acid in the mixture? Oxalic acid and NaOH react according to the following equation: H₂ C₂O4 (aq) + 2 NaOH(aq) → Na2C₂O4 (aq) + 2 H₂O(l) %

You have a mixture of oxalic acid, H₂C2O4, and another solid that does not react with sodium hydroxide. If 25.52 mL of 0.580 M NaOH is required to titrate the oxalic acid in the 4.207 g sample to the second equivalence point, what is the mass percent of oxalic acid in the mixture? Oxalic acid and NaOH react according to the following equation: H₂ C₂O4 (aq) + 2 NaOH(aq) → Na2C₂O4 (aq) + 2 H₂O(l) %

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...

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A student is given 0.716 g of an unknown acid, which can be either oxalic acid, H2C2O4, or citric acid, H3C6H5O7. To determine which acid she has, she titrates the unknown acid with 0.430 M NaOH. The equivalence point is reached when 37.0 mL are added. Answer the following questions to determine the identity of the unknown acid. -How many moles of NaOH are consumed? Moles of NaOH = ____ mol -How many moles of H+ acid are available to react if the acid is H2C2O4? 0.0403 mol NaOH Moles of H+ from H2C2O4 = ___ mol -How many moles of H+ are available to react if the acid is H3C6H5O7? 0.0403 mol NaOH 0.0573 mol H+ from H2C2O4 Moles of H+ from H3C6H5O7 = ___ mol
Chromic acid, H2CrO4, is used in ceramic glazes and colored glass, and is particularly effective for cleaning insoluble organic residues off laboratory glassware. A 10.0 mL sample of chromic acid solution contains 46.0 mg chromium (which is found in the chromic acid). What volume (in mL) of 0.0700 M KOH is needed to neutralize the 10.0 mL sample of chromic acid?
A 0.450 g sample of impure CaCO3(s) is dissolved in 50.0 mL of 0.150 M HCl(aq). The equation for the reaction is CaCO3(s) + 2HCl(aq) - CaCl2(aq) + H2O(l) + CO2(g) The excess HCl(aq) is titrated by 5.60 mL of 0.125 M NaOH(aq). Calculate the mass percentage of CaCO3(s) in the sample. mass percentage:
Write a balanced molecular equation for the reaction that occurs when aqueous solutions of sodium hydroxide, NaOH, and hydrochloric acid, HCl, are combined. It is not necessary to include states such as (aq) or (g). + +
Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq)+NaHCO3(aq)→NaCl(aq)+H2O(l)+CO2(g) The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 50.mL of a 0.027M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.
An aqueous solution of Ca(OH)2with a concentration of 0.188 M was used to titrate 25.00 mL of aqueous HCl. 18.63 mL of the Ca(OH)2was required to reach the endpoint of the titration. How many moles of base were required to react completely with the acid in this reaction? How many moles of HCl were present in the original 25.00 mL of acid?
Sodium hydrogen carbonate NaHCO3 , also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl (aq) + NaHCO3 (aq) → NaCl (aq) + H2O (l) + CO2 (g)The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 50.mL of a 0.081 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits.
A student tries to determine experimentally the molar mass of aspirin (HAsp).She takes 1.00 g of aspirin, dissolves it in water, and neutralizes it with 17.6 mL of 0.315 M KOH. The equation for the reaction is:HAsp(aq) + OH-(aq) ----> Asp-(aq) + H2O(l) What is the molar mass of aspirin?
Sodium hydrogen carbonate NaHCO3 , also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl (aq) + NaHCO3 (aq) → NaCl (aq) + H2O (l) + CO2 (g)The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 150.mL of a 0.045 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits.
Calculate the molar concentration HCl when 250 mL of 0.10 M HCl is mixed with 150 mL of 0.10 M NaOH in a beaker. HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
Molarity of vinegar solution is .8 M
Given: .006718 moles of KHP molarity of NaOH = .3076