Table 4. Calculations for standardization of sodium hyroxideTrial 1Trial 2Trial 3[1] Tared mass of KHCgH,04 (g)0.3740.3250.357[2] Burette reading of NaOH, initial (mL)4.593.614.03[3] Burette reading of NaOH, final (mL)22.0318.7721.17[4] Volume of NAOH, dispensed (mL)[5] Molar concentration of NaOH (mol/L)(2pts) Average molar concentration of NaOH (mol/L) OoldtionTable 1. Measurements for standardization of NaOHTrial 1Trial 2Trial 31] Tared mass of KHC3H4O4 (9)0.3740.3250.35712] Burette reading of NaOH, initial (mL)4.593.614.03[3] Burette reading of NaOH, final (mL)22.0318.7721.17Part B. Molar Concentration of an Acid SolutionEnter the number corresponding to the type of acid you have1. HA32. H2A3. H3AEnter the unknown number.21Table 2. Measurements for titration of unknown acidTrial 1Trial 2Trial 3[1] Volume of acid (mL)25.025.025.0[2] Burette reading of NaOH, initial (mL)2.132.483.68[3] Burette reading of NaOH, final (mL)24.1024.5225.56Part C. Percentage by Mass of an Unknown SolidEnter the number corresponding to the type of acid you have1. HA32. H2A3. H3AEnter the unknown number.30Molar mass of the unknown acid192.14Table 3. Measurements for titriation of solidTrial 1Trial 2Trial 3[1] Mass of sample (g)26.33429.15727.111[2] Burette reading of NaOH, initial (mL)3.211.481.22[3] Burette reading of NaOH, final (mL)22.7723.4220.99

We have to find the molarity of NaOH using moles of KHP

Table 4. Calculations for standardization of sodium hyroxide Trial 1 Trial 2 Trial 3 [1] Tared mass of KHC,H,0, (g) 0.374 0.325 0.357 [2] Burette reading of NaOH, initial (mL) 4.59 3.61 4.03 [3] Burette reading of NaOH, final (mL) 22.03 18.77 21.17 [4] Volume of NaOH, dispensed (mL) [5] Molar concentration of NaOH (mol/L) (2pts) Average molar concentration of NaOH (mol/L)

Table 4. Calculations for standardization of sodium hyroxide Trial 1 Trial 2 Trial 3 [1] Tared mass of KHC,H,0, (g) 0.374 0.325 0.357 [2] Burette reading of NaOH, initial (mL) 4.59 3.61 4.03 [3] Burette reading of NaOH, final (mL) 22.03 18.77 21.17 [4] Volume of NaOH, dispensed (mL) [5] Molar concentration of NaOH (mol/L) (2pts) Average molar concentration of NaOH (mol/L)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter8: Sampling, Standardization, And Calibration

Section: Chapter Questions

Problem 8.17QAP

See similar textbooks

Similar questions

A volumetric calcium analysis on triplicate samples of the blood serum of a patient believed to be suffering from a hyperparathyroid condition produced the following data: mmol Ca/L = 3.55, 3.65, 3.14. What is the 95% confidence interval for the mean of the data, assuming(a) No prior information about the precision of the analysis?(b) s → σ = 0.056 mmol Ca/L?
1. 500.0 mL 0.2 M KI2. 500.0 mL 0.2 M KCl3. 500.0 mL 0.1 M K2S2O84. 500.0 mL 0.1 M K2SO45. 500.0 mL 4.0 mM Na2S2O3 (from Na2S2O3∙5H2O)pls compelete the 2nd table given the data
A mixture containing only Al2O3 (FM 101.96) and Fe2O3 (FM 159.69) weighs 2.019 g. When heated under a stream of H2, the Al2O3 is unchanged, but the Fe2O3is converted to metallic Fe plus H2O(g). If the residue weighs 1.774 g, what is the weight percent of Al2O3 in the original mixture?
pls complete the 2nd table given the data1. 500.0 mL 0.2 M KI2. 500.0 mL 0.2 M KCl3. 500.0 mL 0.1 M K2S2O84. 500.0 mL 0.1 M K2SO45. 500.0 mL 4.0 mM Na2S2O3 (from Na2S2O3∙5H2O)
A mixture containing only Al2O3 (FM 101.96) and Fe2O3 (FM 159.69) weighs 2.019 g. When heated under a stream of H2, the Al2O3 is unchanged, but the Fe2O3 is converted to metallic Fe plus H2O(g). If the residue weighs 1.774 g, what is the weight percent of Al2O3 in the original mixture? (Do not include % symbol in your answer.)
Calcium Chloride Ammonium Chloride Trial 1 Trial 2 Trial 3 Trial 1 Trial 2 Trial 3 Mass of water 100g 100g 100g 100g 100g 100g Mass of salt 5.36g 10.28g 15.10g 5.29 10.43 15.31 Moles of salt Initial T 21.0 21.0 21.0 20.0 20.0 20.0 Final T 29.6 36.2 43.5 17.1 13.2 10.1 ΔT 8.6 15.2 22.5 -2.9 -6.8 -9.9 ΔH(Joules) ΔH(kj/mol)
Mass of original mixture: 0.280g Mass of naphthalene recovered: 0.160 g Mass of 3-nitroaniline recovered: 0.015 g Mass of benzoic acid recovered: 0.135 g 1. a) calculate % by mass of naphthalene, 3-nitroaniline and benzoic acid in original sample 1. b) calculate total mass of three recovered components (g) 1. c) calculate total percent recovery (%)
Beaker 0.00200 M Fe(NO3)3, mL 0.00200 M NaSCN, mL total volume, mL 1 3.000 2.000 10.00 2 3.000 3.000 10.00 3 3.000 4.000 10.00 4 3.000 5.000 10.00 5 (blank) 3.000 0.000 10.00 In Solutions 1-4 you are adding successively larger volumes of 0.00200M SCN- to the Fe3+ solution and diluting to 10.00 ml. Calculate the final diluted molarity of SCN- in solution #1 Your answer should have 3 sig figs =
The percentage of an additive in gasoline was measured six times with the following results: 0.13; 0.12; 0.16; 0.17; 0.20 and 0.11%. What is the 99% confidence interval for the additive percentage?
What is the average ratio in this chart? Please show me the calculation too! Sample 1 2 3 Calculations for sample 1 Mass of aluminum dish 1.24g 1.26g 1.24g - Mass of aluminum dish + Epsom salt 1.70g 1.94g 1.80g - Epsom salt, original (hydrated) mass 0.46g 0.68g 0.56g 1.70g – 1.24g = 0.46g Mass of aluminum dish + Epsom salt after heating 1.42g 1.62g 1.61g Epsom salt, heated (dehydrated) mass 0.18g 0.36g 0.37g 1.42g- 1.24g = 0.18g Mass of water 0.28g 0.32g 0.19g 0.46g – 0.18g = 0.28g Moles of magnesium sulfate 0.0015mol 0.0030mol 0.0031mol 0.18g x (1mol/120.37g)= 0.0015mol Moles of water 0.016mol 0.018mol 0.011mol 0.28g x (1mol/18.02g) = 0.016mol Ratio of moles water: moles of magnesium sulfate 32:3 18:3 11:3.1 0.016 : 0.0015= 32:3 Average Ratio
To determine the mass of Fe2O3 from the given mass of K3Fe(CN)6, the gravimetric factor to be used is a. Fe2O3 / K3Fe(CN)6 b. Fe2O3 / 2K3Fe(CN)6 c. 2Fe2O3 / K3Fe(CN)6 d. 3Fe2O3 / 2K3Fe(CN)6
2H+ + Na2CO3⟶2Na+ + H2O + CO2 the volume of 28.30 ± 0.06 mL of HNO3 solution was required for complete reaction with 0.8450 ± 0.0009 g of Na2CO3, (FM 105.988 ± 0.001 g/mol). Please Find the molarity of the HNO3 solution along with its absolute uncertainty. 1. [HNO3] = ________________ M 2. ___ ± ____________ M