Lab 7 acid base

Calculate the percentage CH3COOH in a sample of vinegar from the following data.Sample = 15.00 g,    NaOH used = 43.00 ml ;   0.600 N H2SO4 used for back titration =0.250 ml  ; 1.00ml NaOH is equivalent  to 0.0315 g H2C2O4. 2H2O.

5. A typical aspirin tablet contains 325mg of acetylsalicylic acid (HC9H7O04) which is a weak acid. The Ka of this acid is 3.69 x 10-4. a. Give the equation for dissociation of the weak acid HC9H7O4. b. What is the initial concentration, in units of molarity, of acetylsalicylic acid if 2 tablets are dissolved in 500. mL of water? c. What is the equilibrium concentration of all species of this solution of acetylsalicylic acid? d. What is the pH, pOH, and % ionization of this solution?

To best accurately determine the molarity of a base, a scientist would need the following: An Erlenmeyer flask, a weighed solid primary standard acid, and NaOH A buret, a weighed solid monobasic base, and an indicator A buret, a weighed solid primary standard acid, and an indicator A buret, a weighed solid primary standard acid, and NaOH A graduated cylinder, a weighed solid primary standard acid, and an indicator

An aqueous solution is made of the diprotic acid H2A to a concentration of 0.15 M H2A. Ka1 = 3.0 x 10-4 and Ka2 = 2.5 x 10-9 What is the [A2-] in this solution? Your answer should have 2 significant figures and be expressed in scientific notation (i.e. 3.0 x 10-2 as 3.0e-2)

Determine the initial concentrations of the species below, after the solutions are mixed. Volume0.0350 MKMnO4(mL)   Volume0.0650 MH2C2O4(mL)   VolumeH2O(mL)   InitialConcentrationKMnO4(M)   InitialConcentrationH2C2O4(M)              (3 significant figures)    (3 significant figures) 1.00   1.00   18.00         2.00   2.00   16.00         3.00   3.00   14.00         4.00   4.00   12.00         5.00   5.00   10.00

For question 5 could you find the best value and explain how you arrive to the best value please thank you!

Please answer Q1

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…

Gg.80.

Suppose a 0.027 M aqueous solution of oxalic acid (H₂C₂O4) is prepared. Calculate the equilibrium molarity of C₂04. You'll find information on the properties of oxalic acid in the ALEKS Data resource. Round your answer to 2 significant digits. M 0 S ? OFF olo

2:10 2- 3C₂²- + 1 2 3 4 N Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. NH3(aq) + HCl(aq) (s) Question 1 of 10 O Reset LO 5 OH H₂O 6 CI 7 6 个 x H₂O Tap here or pull up for additional resources Submit 8 9 11 (aq) O H H3O+

With the image attached write the objective of the experiment in one paragraph Write more than one sentence please

In a 0.60 mM aqueous solution of acetic acid (CH,CO,H), what is the percentage of acetic acid that is dissociated? You can find some data that is useful for solving this problem in the ALEKS Data resource. Round your answer to 2 significant digits. | % x10

I am getting the wrong amount of sig figs for each equation, even though I am using the smallest amount given. May you please solve so that I can see the steps?

300 37-613 *100 = $4.25 7. Base your calculations on the following balanced neutralization reaction: H₂SO4 + 2NaOH → Na2SO4 + 2H₂O a) If you have 35.0mL of 0.50M H₂SO4, how many moles of H₂SO4 do you have? 1.6285 b) If you have 45.0mL of 0.60M NaOH, how many moles of NaOH do you have? c) Based on the balanced equation above, which reactant is the Limiting Reactant? concept: Explain your answer using either calculations d) How many moles of the excess reactant will remain? e) How many molecules of water are produced in the reaction above?

Suppose a 0.027 M aqueous solution of oxalic acid (H₂C₂O) is prepared. Calculate the equilibrium molarity of C₂O You'll find information on the properties of oxalic acid in the ALEKS Data resource. Round your answer to 2 significant digits. M 0.9 X 5

Suppose a student performed a similar standardization titration experiment. Below is the calculated concentration of NaOH from each of their titrations.   Titration #1 Titration #2 Titration #3 The concentration of NaOH (M) 0.9554 0.9540 0.9551 Using the 3 concentrations, calculate the average concentration of the student's NaOH solution and calculate the ± error in parts per thousand (ppt). Show the complete calculation. Express your final answer in the form of average (with units) ± error in ppt.

3. Titration: Strong Acid / Weak Base. (I warned you to be ready!) Here's the cool chart! Analyte: 20.00 mL 0.100 M Hydrazine (N₂H4) Hd A: initial Vertical (Value) Axis Title 0 B: half equivalence C: equivalence 5 10 15 20 Titrant: mL of 0.100 M HCI added 25 20.00 mL of 0.100 M hydrazine (N₂H4, pKb = 5.77) is titrated with 0.100 M HCl. a) Find the initial pH (point A) and the pH at the equivalence point (point C). b) Find the pH at the half equivalence point (point B).

You collected the following data from a titration experiment using a 0.123M standardized NaOH solution to titrate a 27.36 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Initial Final Vol Acid Burette Burette Delivered Concentration Reading (mL) Reading (mL) (mL) (M) Trial 1 0.56 19.20 ?? Trial 2 0.57 19.7 Trial 3 0.92 19.56 For just Trial 1, determine the Molarity concentration of the H2SO4 to 3 significant digits. Do not include units. Answer:

Please send me the questions in 20 minutes it's very urgent plz

Suppose a student performed a similar standardization titration experiment. Below is the calculated concentration of NaOH from each of their titrations.   Titration #1 Titration #2 Titration #3 Concentration of NaOH (M) 0.9554 0.9540 0.9551 Using the 3 concentrations, calculate the average concentration of the student's NaOH solution and calculate the ± error in parts per thousand (ppt). Show the complete calculation. Express your final answer in the form of average (with units) ± error in ppt. use the right significant figures