Calculate :1)Mean Experimental solubility of calcium hydroxide 2)standard deviation3)RSD(pph) Concentration of Hydrochloric Acid (M)0.0703622°cTemperature (°C)Titration 3Titration 1Titration 2Volume of Saturated Calcium10:00ml38.544.66.10l0:00 ml17.710.00ml24.733.6890Hydroxide (mL)Initial Burette Reading (mL)Final Burette Reading (mL)Volume of Hydrochloric Acid (mL)7:009:0004.9196000049752 0:0006262.2:000429196 0.000492520.0429196 0.042952 006262Moles of Hydrochloric Acid (moles)Moles of Hydroxide (moles)0.000 6262Concentration of Hydroxide (M)Concentration of Calcium Hvdroxide0.02146M 0:024626M0.0313IM74g/msl(М)743/mol749/malFormula mass of Ca(OH)2 (g/mol)Experimental Solubility of CalciumHydroxide (g L')2.317g1.58891.82239Mean Experimental Solubility of Calcium Hydroxide (g L')Standard Deviation (g L)RSD (pph)1.5Literature Solubility for calcium Hydroxide' (g L)uiul homical ndf

We can calculate mean, standard deviation and RSD either using a spreadsheet or by using formulas as…

Concentration of Hydrochloric Acid (M) 0.07036 2 2°c Temperature (°C) Titration 3 Titration 1 Titration 2 Volume of Saturated Calcium 10:00ml 38.5 l0:00 ml 10.00'ml 24.7 33.6 8190 Hydroxide (mL) Initial Burette Reading (mL) 17.7 Final Burette Reading (mL) Volume of Hydrochloric Acid (mL) 6.10 7:00 9:0004.91960.00049252 0:0006262. p000229196 lの00049252 10000 6262 0.0429196 0.042952 0:06262 Moles of Hydrochloric Acid (moles ) Moles of Hydroxide (moles) Concentration of Hydroxide (M) Concentration of Calcium Hydroxide b.02146M 743/mol 0:024626M0.03131M 749/mol (М) Formula mass of Ca(OH)2 (g/mol) 749/mal Experimental Solubility of Calcium Hydroxide (g L') 2:3179 1.5889 1.82239 Mean Experimental Solubility of Calcium Hydroxide (g L) Standard Deviation (g L-') RSD (pph) Literature Solubility for calcium Hydroxide' (g L) l ndf 1.5

Concentration of Hydrochloric Acid (M) 0.07036 2 2°c Temperature (°C) Titration 3 Titration 1 Titration 2 Volume of Saturated Calcium 10:00ml 38.5 l0:00 ml 10.00'ml 24.7 33.6 8190 Hydroxide (mL) Initial Burette Reading (mL) 17.7 Final Burette Reading (mL) Volume of Hydrochloric Acid (mL) 6.10 7:00 9:0004.91960.00049252 0:0006262. p000229196 lの00049252 10000 6262 0.0429196 0.042952 0:06262 Moles of Hydrochloric Acid (moles ) Moles of Hydroxide (moles) Concentration of Hydroxide (M) Concentration of Calcium Hydroxide b.02146M 743/mol 0:024626M0.03131M 749/mol (М) Formula mass of Ca(OH)2 (g/mol) 749/mal Experimental Solubility of Calcium Hydroxide (g L') 2:3179 1.5889 1.82239 Mean Experimental Solubility of Calcium Hydroxide (g L) Standard Deviation (g L-') RSD (pph) Literature Solubility for calcium Hydroxide' (g L) l ndf 1.5

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 37QAP: Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at...

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Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
A titration system is set up as follows: the bottom flask contains a sample solution of 50.0-mL 0.50 M C2H3NH2(ethylamine), the burette is filled with 0.20 M HCl as titrant. Kb of C2H3NH2 = 6.5 ´ 10-4 what is the pH at the equivalent point?
it is time for the titration. You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated cylinder and add it to a 125-mL Erlenmeyer flask. Then you add two drops of the indicator, phenolphthalein, to the oxalic acid solution in the flask. You dispense the NaOH solution from the buret into the flask (while swirling the flask) until you reach the endpoint. At the endpoint, the solution in the flask turns light pink. You repeat the titration two additional times for a total of three trials. H2C2O4 (aq) + 2 NaOH (aq) --> Na2C2O4 (aq) + 2 H2O (l) (I) (II) (III) Volume of H2C2O4 used 15.00 mL 15.00 mL 15.00 mL Initial Buret Reading 0.00 mL 0.05 mL 0.10 mL Final Buret Reading 14.45 mL 14.38 mL 15.40 mL what Volume of NaOH is used ?
it is time for the titration. You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated cylinder and add it to a 125-mL Erlenmeyer flask. Then you add two drops of the indicator, phenolphthalein, to the oxalic acid solution in the flask. You dispense the NaOH solution from the buret into the flask (while swirling the flask) until you reach the endpoint. At the endpoint, the solution in the flask turns light pink. You repeat the titration two additional times for a total of three trials. H2C2O4 (aq) + 2 NaOH (aq) --> Na2C2O4 (aq) + 2 H2O (l) (I) (II) (III) Volume of H2C2O4 used 15.00 mL 15.00 mL 15.00 mL Initial Buret Reading 0.00 mL 0.05 mL 0.10 mL Final Buret Reading 14.45 mL 14.38 mL 15.40 mL Volume NaOH used ________mL ________mL ______mL Moles NaOH _______M ________M _________M…
A commercial vinegar was analyzed by titration to determine the percent acetic acid. Briefly, 10.00 mL of vinegar sample was diluted to 100. mL solution in a volumetric flask. A 25.00 mL aliquot from the diluted vinegar required 25.55 mL of 0.1005 M sodium hydroxide to reach the phenolphthalein endpoint From this experiment which is the standard solution used in titration? CH3COOH NaOH NaCH3COO C20H14O4
Calculate the number of moles of acetic acid in 100mL of both samples of vinegar accurately titrated. given: NaOH vs CH3COOH Burette solution is NaOH and the pipette solution is 5.0 mL of Vinegar Titration Initial burette reading Final burette reading Volume of NaOH consumed Average volume of NaOH Approximate 0.0 mL 20.1 mL 20.1 mL 20.3 mL Titration 1 0.0 mL 20.9 mL 20.9 mL Titration 2 0.0 mL 20.0 mL 20.0 mL To find the average volume Average volume = 20.1 mL + 20.9 mL + 20.0 mL320.1 mL + 20.9 mL + 20.0 mL3 = 20.3 mL Concentration of Vinegar = Volume of NaOH * Concentration of NaOHVolume of vinegarVolume of NaOH * Concentration of NaOHVolume of vinegar = 20.3 mL * 0.0647 M5.0 mL20.3 mL * 0.0647 M5.0 mL = 0.2627 M Concentration of NaOH = Volume of H2SO4 * Concentration of H2SO4Volume of NaOHVolume of H2SO4 * Concentration of H2SO4Volume of NaOH…
An automatic titration of Cola product was analyzed and the following results were produced: Volume of Standardized NaOH Titrant used to achieve the first equivalence point in titration: Trial #1: 1.300 mL Trial #2: 1.137 mL Trial #3: 1.140 mL May you explain why trial #1 was skewed; for example, if pipetting of the 25.00 mL was done incorrectly, how would the molarity change if the volume examined was supposed to be 24.50 mL?
A student performed titration to determine the concentration of potassium permanganate solution with oxalic acid. The net ionic equation is as follows: 2MnO4– + 16H+ + 5C2O42- → 2Mn2+ + 10CO2 + 8H2O The titration consumed 42.31 mL of 0.1001 M oxalate solution to reach the endpoint. Determine the concentration of permanganate (M) if 25 mL was used.
1 ) The density of a 5.26MNaHCO 3 (84.0 g/mol) is 1.19g / m * l . Its molality is 2) Calculate the pAg^ + at the equivalence point in the titration of 25.0ml of 0.0823 M Kl with 0.051M AgNO 3 . Ksp Agl=8.3*10^ -16 3) Commercial concentrated aqueous nitric acid is 70.4% HNO3(63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is 4) Consider the titration of 25ml of 0.0823M KI with 0.051M AGNO3, Kspagi =8.3x10-16 Calculate pAg* after adding 39.0 ml I03 Ag* + 103 ====AglO3 5) Commercial concentrated aqueous nitric acid is 70.4 1\%HNO 3 (63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is: 6) What mass in g of Na 2 CO 3 [106 g/mol] is required to prepare 250 ml of 0.3M aqueous solution in Na^ + [23.g/mol] ? 7) Calculate pAg^ + after adding 42.30ml AgNO 3 In the titration of of 0.0823M Kl with 0.051M AgNO 3 . KspAgl = 8.3 * 10 ^ - 16 8) The milliliters of concentrated HClO 4 (100.5 g/mol),6 60% by mass,…
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A titration system is set up as follows: the bottom flask contains a sample solution of 50.0-mL 0.50 M C2H3NH2 (ethylamine), the burette is filled with 0.20 M HCl as titrant. Kb of C2H3NH2 = 6.5 ´ 10-4 What is the initial pH of above sample solution before titration starts?
A student weighs a sample of potassium hydrogen phthalate (KHP) to prepare a primary standard for a titration. She later discovers that the KHP was contaminated with sugar. To determine the amount of KHP in the mixture, she takes 4.678 g4.678 g of the mixture and make a 100.0 mL100.0 mL solution. The student then titrates 10.00 mL10.00 mL of this solution with a 0.1030 M0.1030 M sodium hydroxide solution. She finds that 15.15 mL15.15 mL of the NaOHNaOH solution is needed to reach the end point.