post lab 6 and 7

Based on this student data, calculate the average molarity of the NaOH solution. Standard: KHP = potassium hydrogen phthalate, MM 204.4 g/mol Student Data Trial 1 E KHP mL initial: NaOH mL final: NaOH 2.02 0.57 19.25 Trial 2 2.05 19.25 39.80 Trial 3 1.99 1.65 20.75

What is the purity test of salicylic acid and commercial aspirin?

What are the Volumes of HCl from the 3 Trials?

Standard Sodium Chloride Weighed mass of NaCI g in 250.0 mL Purity of NaCl = 100.03 % Molar concentration of NaCl using weighed mass and purity mol L-1 Titrations of standard NaCI (25.00 ml aliquots) with the provided AGNO3 Precise Titration # Volume of AGNO3 required (mL) 1 2 3.

What is the purity test of synthesized aspirin and commercial aspirin?

A solution is initially 0.10 M in Mg2*(aq) and 0.10 M in Fe2* Mg(OH)2 first precipitates? Ksp (Mg(OH)2) = 6.0 x 10-10; Ksp(Fe(OH)2) = 7.9 x 10-16 your answer in E-notation, rounded to 2 significant digits. *(aq). A solution of NaOH is slowly added. What is the concentration of Fe2+ when %3D Provide

Titration of Acetic Acid CH3COOH 1) Record the exact Molarity of the freshly prepared solution of NaOH by reading the label on the bottle, include all digits provided. This is the solution that will be in the buret. MB 0.0500 M 2) Record the exact volume of acid CH,COOH that was pipetted into the Erlenmeyer 10.00 aak mL. Note the concentration is unknown and what you will solve for. (This was diluted with 50 mL of water in the Erlenmeyer flask) Trial 1 Trial 2 Trial 3 Final base (mL) 30.46 30.98 29.88 Initial basc (mL) 0.45 0.05 0.04 Total base (mL) *Molarity (M) HOOD HO "Use atoichiometry to determine the molarity of your CIHCOOH solution fromn each of trial. Show all work Including units for one. Caleulate Average Molarity

Pretend that you are conducting this experiment in the laboratory and answer the following questions. You are asked to weigh 2 g of  lithium and add it to 1500 ml of distilled water +2 drops of indicator, knowing that the density of water is 1 at room temperature while conducting this experiment. After knowing the amount of LiOH, you need to dilute to prepare 0.025 M of LiOH in a 3000 ml(v) solution. Show your calculation  and units.Knowing that the initial volume that you used was 1500 ml(v).  Use this equation to calculate ( CLiOH x VLiOH) before dilution =  (CLiOH x VLiOH) after dilution

(1) Careless Carlie weighed her KHP sample, but forgot to bring her report sheet along, so she recorded the mass of KHP on a paper towel. During her titration, which required 18.46 mL of base, she spilled some base on her hands. She remembered to wash her hands, but forgot about the data on the towel, and used it to dry her hands. When she went to calculate the molarity of the base, Carlie discovered that she didn’t have the mass of her KHP. Her kindhearted instructor told Carlie that her base was 0.2987 M. Calculate the mass of Carlie’s KHP sample. Show calculations       (2) What mass of solid NaOH would be needed to make 645 mL of Carlie’s NaOH solution? Show calculations.

The following volumes of 0.000300 M SCN- are diluted to 15.00 mL. Determine the concentration of SCN- in each sample after dilution. These values will be used during the experiment.  Sample 0.000300 M SCN- (mL) [SCN-] (M) 1  1.50   2 3.50   3 7.00   4 10.00

EXPERIMENT 5; Acid-Base Titration A. Trial 1 Trial 2 Trial 3 5.210 g Mass of KHP 5.210 g 5.210 g (C3H,O4) Mole of KHP Initial Burette 0.00 0.50 5.00 Volume NaOH (mL) Final Burette 31.00 26.25 29.95 Volume NaOH (mL) Total Volume of NaOH (mL) Moles of NaOH Molarity of NaOH (mol/L) Calculate the average Molarity of NaOH B. Titration of Vinegar (HC,H3O2) A 2.352 g sample of Vinegar is titrated with 0.08751M NaOH, and it requires 22.31 mL of NaOH to reach the endpoint. Calculate the mass percent of acetic acid (HC,H;O,) in the vinegar sample? Hint for Calculation of Mass percent of Vinegar (HC,H;O2) 1. Calculate mole of HC,H;O2 from concentration (M) and volume of NaOH (L) needed to titrate Vinegar 2. Calculate mass (g) of Vinegar from mole of Vinegar 3. Mass % Vinegar = (calculated mass Vinegar/ 2.352 g) X 100 C. A solution of malonic acid, H;C;H¿O4 ¸was standardized by titration with 0.100 M NaOH solution. If 20.76 mL of the NaOH solution were required to neutralize completely 13.15 mL of…

I need help calculating the values of the molarity of KMnO4 solution and the averages please. reaction equation --> 2 MnO4− + 5 C2O42− + 16 H+ → 2 Mn2+ + 10 CO2 + 8 H2O

< Question 12 of 17 A 25.0 mL solution of HNO3 is neutralized with 25.4 mL of 0.250 M Ba(OH)2. What is the concentration of the original HNO3 solution? Tap here or pull up for additional resources 1 4 7 +/- M 2580 3690 . X C x 10

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A student, performing the same experiment as you, recorded the following information. The original solution was diluted by a factor of 5.Calculate the volume of NaOH used to reach the equivalence point. Volume of diluted vinegar sample (mL)     25.00 Molarity of NaOH                                       0.0900 Initial buret reading (mL)                            16.50 Final buret reading (mL)                             38.00 Volume of NaOH

Based on the analysis of a vinegar solution via titration with 0.1 M NaOH. Results are as follows: Trial 1 Volume of vinegar solution used (mL) 5.00 Final burette reading (mL) 44.20 Initial burette reading (mL) 0.00 Determine the percentage mass of acetic acid in vinegar for Trial 1. The density of vinegar is 1.01 g/mL and molecular mass for acetic acid is 60 g/mol.