6. During titration, an aqeous solution of HCI has a concentration of 0.1396 mol dm. If24.71 cm (24.71 m) of this solution is delivered from a buret, what amount of HCI hasbeen delivered?a) 0.1396 mol/Lb) 0.1490 mol/Lc) 0.169 mol/Ld) 0.1265 mol/L7. Exact amount of 25.0 ml NaOH solution whose concentration is 0.974 M was deliveredfrom a pipet.a) What amount of NaOH was present?a) 2.66 X 10° molb) 2.44 X 10° molc) 2.0 X 103d) 3.6 X 103 mol

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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

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

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Example: Vinegar is an aqueous solution of acetic acid, HC₂H₂O₂ (HAc). A 12.5 mL sample of vinegar was titrated with a 0.504 M solution of NaOH. The titration required 15.40 mL of the NaOH solution to reach the endpoint. What is the concentration of HAc in vinegar?
5. A student conducted a titration experiment. He/she used 12.0 mL of silver nitrate (titrant) solution to reach the endpoint. If the student used 25.4 mL of the chloride (analyte) for the titration and found the concentration of chloride ions to be 2.2 M, what is the mass (in grams) of silver nitrate titrant Clic)
solution after precipitation is complete. 68. The drawings below represent aqueous solutions. Solution A is 2.00 L of a 2.00-M aqueous solution of copper(II) nitrate. Solution B is 2.00 L of a 3.00-M aqueous solution of potas- sium hydroxide. (0) suiro Cu²+ ebro NO3 БО K+ OH™ A B a. Draw a picture of the solution made by mixing solutions A and B together after the precipitation reaction takes place. Make sure this picture shows the correct relative volume compared to solutions A and B, and the correct relative number of ions, along with the correct relative amount of solid formed. b. Determine the concentrations (in M) of all ions left in solution (from part a) and the mass of solid formed.
A titration was performed using 0.985 M NaOH to determine the molarity of a HCI solution. The volume of HCI was 25.0 mL. The volume of NaOH in the buret before titrating was 12.90. After the titration, the NaOH volume in the buret was 37.35 mL. What is the molarity of the HCi solution?
Consider the titrimetric determination of acetic acid (60.05 g/mol) in vinegar. Titration of a 5.00 mL vinegar sample requires 16.15 mL of 0.250 M NaOH to reach the phenolphthalein end point. What is the percent weight by volume of acetic acid in the sample? 2.97 4.85 6.01 7.44 None of the choices
Consider the neutralization reaction 2 HNO3(aq) + Ba(OH)2(aq). 2 H2O(l) + Ba(NO3)2(aq) A 0.105 L sample of an unknown HNO3 solution required 42.5 mL of 0.250 M Ba(OH)2 for complete neutralization. Wha the concentration of the HNO3 solution? concentration: .098
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1166 M standard sodium hydroxide solution. He takes a 25.00mL sample of the original acid solution and diluted it to a 250.0mL. Then, he takes a 10.00mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 12.52mL of the standard solution. What is the concentration of the original sulfuric acid solution? concentration:_____M
A solution was made by adding water to 0.293 g of H2ZH2Z until the volume totaled 25.00 mL. Subsequent titration required 40.50 mL of 0.093 M sodium hydroxide. Calculate the molar mass of H2ZH2Z (in g/mol).
One of the main acidic components of acid rain is sulfuric acid, H₂SO4. Assuming sulfuric acid is the only acid in the acid rain, what volume (in mL) of 0.000915 M KOH would be required to titrate a 45.00 mL sample of acid rain with an H₂SO4 concentration of 1.230 × 10-4 M? Volume mL
One method of determining the concentration of hydrogen peroxide (H₂O₂) in a solution is through titration with iodide ion. The unbalanced net ionic equation for this reaction is H₂O₂ +1+H* → 1₂ + H₂O A 50.00 mL sample of a hydrogen peroxide solution is found to react completely with 37.12 mL of a 0.1500 M KI solution. What is the concentration of hydrogen peroxide in the sample? O a. 0.2227 M O b. 0.4041 M O c. 0.1010 M O d. 5.568 x 10-² M 17.5 mL of a 0.1050 M Na₂CO3 solution is added to 46.0 mL of 0.1250 M NaCl. What is the concentration of sodium ion in the final solution? O a. 0.119 M O b. 0.148 M O c. 0.539 M O d. 0.205 M
d) A 38.5mL sample of 0.875M AgNO, solution is mixed with 51.0mL sample of 0.744M NaCl solution. The AgCl precipitated has a mass of 2.06g. Calculate the limiting reactant, the theoretical yield, and percent yield. AGNO3(aq) + NaClaq) → AGCI6) + NaNO3(aq)
What volume of 0.0105 -M HBr solution is required to titrate 125 mL of a 0.0100 – M Ca(OH)2 solution? Ca(OH) 2(aq) + 2HBr(aq) → CaBr2(aq)2H2O(1) a. 0.0776 mL b. 24.8 mL c. 77.26 mL d. 0.248 mL

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During titration, an aqeous solution of HCI has a concentration of 0.1396 mol dm. If 24.71 cm (24.71 m) of this solution is delivered from a buret, what amount of HCI has been delivered? a) 0.1396 mol/L b) 0.1490 mol/L c) 0.169 mol/L d) 0.1265 mol/L