Table 1: Standardization DataTrial 1Trial 2O145504Mass of KHP04536Initial burette reading0.05ML12.3MLFinal burette reading12.8a6.omLVolume of base usedר.1213.2 mLData Analysis: KH Cg Hg Da (MOIAR MASS 2041ag)1. Calculate the molarity of base for each trial. You must use dimensional analysis – show all unit conversions(hint: start with grams of KHP used). Review the balanced equation for KHP and NaOH you wrote in Expt 11 part 1.(204.29TRIAI 1: 0.4550g.Average:Trial 2:Trial 1:with 1875 mL of your base (use the average

To calculate the Molarity of base, we would first check the mole ratio between base and KHP from the…

Answered: M: Table 1: Standardization Data Trial…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.20QAP

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The distribution constant for solute Z. between Water is 3.7. Calculate the remaining consentration of 2. remaining in a solution when 0.036 M and 31 ml. aparous solution of A is extracted with 4 portions of 8 ml. hexane AY 7.28 x 10M B ) 7.37 x 10M C) 148 x 10M D) 2.61 x 10M E ) 1.87 x 10M
3.A sample is known to contain NaOH, Na2CO3 NaHCO3 or compatible mixture of these together with inert matter. With methyl orange, a 1.100 g sample requires 31.40 mL of HCl ( 1.00 mL is equivalent to 0.0140g CaO). With phenolphthalein indicator, the same weight of sample requires 13.30mL of the acid. What is the percent composition of the sample? ww ww
K2CO3(aq) + 2HC2H3O2(aq) yields 2KC2H3O2(aq) + H2O(l) + CO2(g) How many moles of H2O can be obtained from 25.0 ml of 0.150 M HC2H3O2?
P UTF-8 Chapter 12 Solutions-20 x+ s.content.blackboardcdn.com/5b19550b0b538/10621560?X-Blackboard-Expiration3164905200001 neet.docx Edits will not be automatically saved. Save now amond A 14 三三三兰 7. What is the molarity of a solution when 2.0 L. of a 6.0 M HCI solution is added to water so that the final volume is 6.0 L? (5 pts) 8. When placed in cach of the following, indicate if a red blood cell will Becrenati (4 pts
How many milliliters of 0.10 M Pb(NO 3 )2 should be used to make ni(en)(h2o)4so4 10% mole excess?
cium chloride per liter. Express the centration in terms of milliequivalents of calcium chloride (CaCl2-2H20-m.w 147) per liter. con- 27. How many milliequivalents/of potassium would be supplied daily by the usual dose (0.3 mL three times a day) of saturated potassium iodide solution? Saturated po- tassium iodide solution contains 100 g of potassium iodide per 100 mL.oluce 28. An intravenous solution calls for the addi- tion of 25 mEq of sodium bicarbonate. How many milli 4%
TITRIMETRIC DATA SAMPLE: CANE VINEGAR % acidity in label: 4.5% %purity of KHP: 99.80% FORMULA WEIGHT of KHP: 204.22 g/mol STANDARDIZATION OF NaOH SOLUTION TRIAL 1 TRIAL 2 TRIAL 3 Weight of KHP, g 0.1012 0.1004 0.09987 Initial volume of NaOH, mL 5.00 10.01 Final volume of NaOH, mL 4.95 9.99 14.93 Molarity of NaOH Average Molarity of NaOH ANALYSIS OF ACETIC ACID IN A VINEGAR SAMPLE TRIAL 1 TRIAL 2 TRIAL 3 Volume of vinegar, mL Initial volume of NaOH, mL 1.00 1.00 1.00 14.98 22.90 30.87 Final volume of NaOH, mL 22.84 30.77 38.75 Molarity of acetic acid Average molarity of acetic acid ANALYSIS OF CARBONIC ACID IN A SODA SAMPLE TRIAL 1 TRIAL 2 TRIAL 3 Volume of soda, mL 20.0 20.0 20.0 Initial volume of NaOH, mL 20.20 22.05 23.93 Final volume of NaOH, mL 22.03 23.89 25.8 Molarity of carbonic acid Average molarity of carbonic acid
2. Calculate the [I] (after dilution in the 50.00 mL flasks) for the four standard solutions you make up in part B. Use the data given in Table B and show all calculations. Round your answers to the correct number of significant figures. Record these values on the spreadsheet template before the lab.
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1. Find the number of millimoles of solute in a. 226 ?? of 0.320 ? HClO4. b. 25.0 ? of 8.05 ? 10−3 ? K2CrO4. c. 6.00 ? of an aqueous solution that contains 6.75 ??? of AgNO3. d. 537 ?? of 0.0200 ? KOH. 2. Describe the preparation of a. 5.00 ? of 0.0500 ? KMnO4 from the solid reagent. b. 4.00 ? of 0.250 ? HClO4, starting with an 8.00 ? solution of the reagent. c. 400 ?? of a solution that is 0.0250 ? in I2, starting with MgI2. d. 200 ?? of 1.00% (?/?) aqueous CuSO4 from a 0.365 ? CuSO4 solution. e. 1.50 ? of 0.215 ? NaOH from the concentrated commercial reagent [50% NaOH (w/w), ?? ?? = 1.525]. f. 1.50 ? of a solution that is 12.0 ??? in K+, starting with solid K4Fe(CN)6. 3. Exactly 75.00 ?? of a 0.3132 ? solution of Na2SO3 were treated with 150.0 ?? of 0.4025 ? HClO4 and boiled to remove the SO2 formed. a. What was the mass in grams of SO2 that was evolved? b. What was the concentration of the unreacted reagent (Na2SO3 or HClO4) after thereaction was complete?
solute 0.147 g C6H7NaO6 molar mass 198.11, dissolves in 50.00 mL, absorbance of solution 0.862, absorbance of standard 0.863 calculate moles of solute, volume of solution (L), %m/v, M, % error

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