Question 4 A student analyzed impure samples of oxalic acid dihydrate (MM= 126.08 g/mol) using a (1.19x10^-1) M solution of NaOH. If a (4.707x10^-1) gram sample of impure acid required (3.788x10^1) mL of NaOH to reach the end point of the titration, how many grams of oxalic acid dihydrate were in the original sample? Enter your answer in scientific notation with three significant figures. Do not include any units in your answer. Note: The numbers in this problem are different from the numbers in other problems. Note: Your answer is assumed to be reduced to the highest power ossible. Your Answer: x10

Question 4 A student analyzed impure samples of oxalic acid dihydrate (MM= 126.08 g/mol) using a (1.19x10^-1) M solution of NaOH. If a (4.707x10^-1) gram sample of impure acid required (3.788x10^1) mL of NaOH to reach the end point of the titration, how many grams of oxalic acid dihydrate were in the original sample? Enter your answer in scientific notation with three significant figures. Do not include any units in your answer. Note: The numbers in this problem are different from the numbers in other problems. Note: Your answer is assumed to be reduced to the highest power ossible. Your Answer: x10

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 121AP: Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion...

See similar textbooks

Similar questions

According to the reaction below: if it required 36.52 mL of H2SO4 with an unknown concentration to completely react with 0.722 grams of NaOH what was the initial concentration of the H2SO4 solution in mol/L ? (This is a titration problem) H2SO4 +2NaOH → 2H2O + Na2SO4
1. If 2.50 mL of vinegar requires 34.90 mL of 0.0960 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in 500.0 mL of this vinegar? [density of vinegar = 1.01 g mL-1] 2. Calculate the mass % of acetic acid in the vinegar in the previous exercise (question#1 above). Assume that the density of the vinegar is 1.01 g mL-1.
Volume of HCL sample = 15ml Molarity standardized NaOh solution = .09929 Initial buret reading = 17.85 mL NaOH final buret reading = 36.16 mL NaOH volume of NaOH used = 17.31 Equation HCl = NaOH=NaCl + H2O What is the molarity of the HCl sample?
1. If 2.50 ml of vinegar requires 34.90 ml of 0.0960 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in 500.0 ml of this vinegar? ( density of vinegar =1.01 g/ml) 2.calculate the % mass of acetic acid in the vinegar in the previous exercise (question #1 above). Assume that the density of the vinegar is 1.01 g/ml 3. If the phenolphthalein is used as indicator, what color will the solution be at the endpoint ? 4. In your reading, it talks about errors that are possible when doing titrations, what are three of those possible sources of error?
KHP + NaOH—> KNaP +H2O Data of trial Mass of KHP : 0.8079g Initial buret containing NaOH reading: 0.05ml Final buret containing NaOH reading : 34.01ml ml of NaOH used: 33.96ml Question 1) calculate the molarity of NaOH
Question: To prepare a new sample from a stock solution, a student pipets 25.00 mL of 1.063 M NaOH solution into an empty 500.0 mL volumetric flask, and then fills the volumetric flask to the line with deionized water. What is the molar concentration of the new solution? I need help with putting the numbers into the formula for this, then I should be able to solve it. Thanks.
In a titration of Vinegar, the average volume of 0.1 M NaOH used after three titrations is 4.26 mL. If the density of vinegar (acetic acid) is 1.006 g/ml and the molecular mass of CH3COOH is 60.05 g/mol. The mass percent (%m/v) of the vinegar is: 5x10-5 5x10-4 0.5 5x10-3
During a titration involving 1.852 g of KHP powder, the amount of NaOH in a buret started at a reading of 3.56 mL & ended at a reading of 28.13 mL. Part C: If the concentration of the NaOH used was 0.300 M, then how many moles of NaOH were dispensed from the buret? Type the answer without using scientific notation.
In 2 liters of a 0.0100 M potassium permanganate solution that we wanted to standardize with a primary standard solution of sodium oxalate, it was planned to use between 30.00 and 45.00 mL of the titrated reagent. Question:In what mass range (in grams) should the primary standard be weighed? Data: Molar Mass of KMnO4 = 158.00 g/mol; Molar Mass Na2C2O4 = 134.00 g/mol
Phosphoric acid, H3PO4, in a solution was neutralized by titration with a barium hydroxide, Ba(OH)2 solution. If 16.2 mL of phosphoric acid solution required 46.1 mL of 0.100 M Ba(OH)2 for neutralization, what was the molarity of the phosphoric acid in the original solution? 2 H3PO4 + 3 Ba(OH)2 → Ba3(PO4)2 + 6 H2O answer is 0.19 but I dont know how to solve it
What is the normality of an acid if 21.18 mL were needed to titrate 0.1369 g Na2CO3?
Need help with question 7 but 4-6 are here for context, thank you. Question 4 A standardized iron (II) solution that is 0.224 M in Fe2+ was used to determine the concentration of permanganate in solution. If the titration required 31.2 mL of Fe2+, how many moles of permanganate ion are present in solution? The pertinent balanced chemical equation is: MnO4- (aq) + 5 Fe2+ (aq) + 8 H+ (aq) --> Mn2+ (aq) + 5 Fe3+ (aq) + 4 H2O (l). Question 5 A standardized iron (II) solution that is 0.224 M in Fe2+ was used to determine the concentration of permanganate in solution. If the titration required 31.2 mL of Fe2+, how many moles of permanganate ion are present in solution? The pertinent balanced chemical equation is: MnO4- (aq) + 5 Fe2+ (aq) + 8 H+ (aq) --> Mn2+ (aq) + 5 Fe3+ (aq) + 4 H2O (l). Question 6 An ore containing solid titanium was processed so that it would yield titanium (IV) permanganate. A titration with an iron (II) standard was performed that indicated that…