CHEM 110L - Experiment 10 It's Back

The flask contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.140 M NAOH. It requires 16.4 mL of the NAOH solution to reach the end point of the titration. What is the initial concentration of HCl? concentration: M HCI about us careers privacy policy terms of use contact us help docx DII F5 PrtScn 8 Home F9 End F10 PgUp F11 F4 F6 F7

Quantity of Acetic Acid in Salad Dressing Titration Results: 1000 μL aliquots of salad dressing against a sodium hydroxide solution Please only fill in 3 concordant results! Titration number: 1 2 3 Error Final burette reading (mL) 7.9 15 22.2 ±0.05 mL Initial burette reading (mL) 0.9 7.9 17 ±0.05 mL Titre (mL) 7 7.1 7.2 ±0.10 mL Average (mean) volume of concordant titres: 7.1 Concentration of Acetic Acid (M) (to 3 sig figs): 6.88 mL IM Concentration of Acetic Acid (as %w/v) (to 3 sig figs): % Note: %w/v = (g/mL) x 100%

14.00 4. A student titrates 20.0 ml of an acid pH vs. Volume NaOH Added 13.00 solution with 0.500 M NaOH and gets the graph shown below. 12.00 Determine the 11.00 concentration of the acid. 10.00 pH 9.00 8.00 7.00 6.00 5.00 4.00 0.0 2.0 4.0 6.0 8.0 10.0 12.0 14.0 Volume of 0.500 M NaOH Added

Calculate the Molarity

3. A student titrates 20.0 ml of an acid solution with 0.500 M NaOH and gets the graph shown below. Determine the concentration of the acid.

A 10.0 mL sample of H₂SO4 is titrated with 0.685 M NaOH. The initial buret volume is 0.10 mL and the final buret volume is 28.92 mL. What is the concentration (mol/L) of the H₂SO4 sample? Answer to 3 decimal places with no units. Your Answer: Answer

From the titrations  below, calculate the molarity  of the NaOH  solution in each of the f ollowing? Make sure you balance the equations.    a) NaOH    + HCl  →  NaCl   + H2O 32.00 ml of NaOH  is required to completely react with 25.00 ml  of 0.150 M HCl.  ___________   b)  NaOH   +    H2SO4   →   Na2SO4  +  H2O 42.00 ml of NaOH  is required to completely react with 18.00 ml  of 0.10M H 2SO4 .  __________

Part A: Standardization of a Sodium Hydroxide Solution   Titration 1 Titration 2 Titration 3 Mass of 125 mL flask 45.849g 46.715g 44.953g Mass of flask and KHP 46.849g 47.745g 46.003g Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 27.8 ml 26.5 ml 26.7 ml Volume of NaOH used (mL) 45.11 ml 45.06 ml 45.14 ml   Calculations   Titration 1 Titration 2 Titration 3 Moles of KHP       Moles of NaOH       Molarity of NaOH         Average Molarity of NaOH: _______________

Titration Calculation Practice 4 1. Nitrous acid has a Ka of 4.0 x 104. Calculate the pH at the following places on a titration curve when 40.00 mL of 0.125 M NANO2 is titrated against 0.200 M HC1. a. the initial pH b. the pH at the point when 12.50 mL acid has been added c. the pH at the point when 15.00 mL acid has been added

It’s a 4 part question

25

55 ml of Na2CO3 solution was titrated with 1.2 M of HCI according to the following reaction Na2CO3 + 2HCI 2NACI + H2CO3 If 27 ml of HCI are required to completely reacts with Na2CO3 solution Calculate the molarity of Na2CO3 solution Select one: O a. 2.5 M O b. 0.3 M O c. 1.8 M O d. 0.6 M O e. 0.9 M

How to calculate the volume used?

Can you please do number 14 III.  Can you tell us how to get the volume.  I want to know how to calculate the volume in this titration of ch3nh2. See pic.. This is not a graded question as it is a practice question . I am 60 years old and helping my son prepare for the AP exam in a few months. We do questions at the back of the textbook by Zumdahl and Zumdahl

Find the number of moles of HCl added.  Concentration of HCl solution, M: 0.60 Initial buret reading: 0.35 ml  Final buret reading: 5.65 ml  Volume of titrant: 5.35 ml

Only typed solution

QUESTION 5 In an experiment, it requires 35 ml of NaOH to titrate 0.35 g of dissolved KHP (molecular weight = 204.22 g/mol) to the phenolphthalein end point. Calculate the concentration of NaOH in mol/L . Оa.4.896 М O b.0.4896 M Ос. 0.490 М O d. 0.0490 M O e. 1.714 M

Please answer true or false

of 36 - Module 8: Ho X om/sac/7086543#/7086543/23/1 e: > 91.7% Question 24 of 35 - Module 7 Ho X pH = x10 TOOLS Topic: Week 4 Discussion h Resources 144 X A volume of 500.0 mL of 0.110 M NaOH is added to 585 mL of 0.250 M weak acid (K, = 8.02 x 10-5). What is the pH of the resulting buffer? HA(aq) + OH(aq) → H₂O(1) + A (aq) + Give Up? DDI Q Hint ☐ Check Answer Attempt 3 12:51 PM 9/29/2022 O Y

In the titration curve shown in Figure 2, the number of data points tends to increase in certain region of the titration curve.  Can you explain when this occurs and why it is a good idea?  Will you adopt this strategy when you are titrating? (The answer to this last question is yes, you will.)

based on the data tables provided, what is % CH3COOH in vinegar