Hello there. I need help with working on some calculations for two vials (with numbers 3 and 6). We did a lab that measured three vials. In vial #1, it had a pH of 9, 5 mL of solution was added, and the moles were 5x10^-8 mol OH-. The actual pH was 6.69 for vial #1.
Calculate the number of moles of either OH- or H3O+ in the solution that was added. (OH-) if the solution was a base or H3O+ if the solution was an acid) and calculate the expected pH of the solution in the vial
Equation: H3O+(aq)+OH-(aq) -> 2H2O(l)
In vial #3, I said it was a base (1.0x10^-11 aka pH of 11) and 1mL of solution was added.
and in vial #6 I said it was an acid (1.0x10^-1 aka pH of 1) and 1mL of solution was added.
I'm lost on how to calculate the moles and then the pH. Below is what I have so far and I would really appreciate some guidance. Thank you!
Hello there. I need help with working on some calculations for two vials (with numbers 3...
please show all work for part III :) all the information needed is in the pictures III. Preparing HC,HO, Solutions and Determining pH only cal. One! theoretical pH 1.0 x 10-14 (181) concentration of HC,H,O, M measured pH ya ? 3.06 1.0 x 10-2 ka: 1. 8x10°3 ixio- 3.43 1.0 x 10-3 x = CH) -1,34% 103n 3.87 1.0 x 107 PM - 04 TH11 4.30 concentration of HC,H,O, M calculated K of HC H302 based on pH data literature...
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pH operates off of a ___________ scale. The autoionization constant of water is abbreviated ________. The molar concentration of hydronium in pure water at 25ºC has been measured to be ________. The relationship between hydronium and hydroxide in any dilute aqueous solution is represented by _________. The p in pH stands for _________. The relationship between pH and pOH is ___________. The pH value of a 1 M solution of strong acid would be...
Please help!! I will rate all answers!! The OH-ion concentration in a certain ammonia solution is 7.2 x 10-M. What is the pOH and pH? Ans: 3.14 and 10.86 What is the H30* ion concentration in a solution with a pOH of 3.9? Ans: 8 x 10-11M The pH of many cola-type soft drinks is about 3.0. a) Calculate the [H3O+] in soft drinks. Ans: 1 x 10-3M b) How many times greater is the H30concentration in these drinks than...
Question two A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 ml solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O2. The initial concentration of both the acid and the base are 0.0100 mol/0.1000...
1. Multiple choice: Each question is worth 4 points (some useful equation are on last page) 1. As ionic strength increases, the values of activity coefficients: a. change randomly C. decrease b. increase d. do not change What is the pH of a solution with (HA) = 0.01M and [A] = 0.01M, when pk, = 5.2? (Assume HA and A) are conjugates. a. 5.2 b. 4.2 C. 6.2 d. 7.0 Which solution has a higher ionic strength? A 0.500M solution...
Need help with 3 and 4 on calculations. some info is on top of the page Data Sheet for Lab #10 Name: Partner: Data/Observations: Volume of (NH), SO, used: Suomi initial pH of (NH4)2SO4 6.79 Equivalence vol. of NaOH: 20.00 pH at half-equivalence: 10,63 Balanced Chemical Equation: 1. Write the balanced equation for the reaction of ammonium sulfate and sodium hydroxide. (NH4)2SO4(s)? 2 N.0H(1) Nasa, () + 2NH3(-) + 2H2O 2. Write the balanced equation showing the ammonium ion acting...
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I need help with #3, 4. Also, I am confused with #5 because both pH are the same. Ka 1-7X10 4 3. In a titration between HCHO, and KOH, would the pH at the equivalence point be acidic, basic, or neutral? Briefly explain your answer. HCHO+KOH b) Which of the following acid-base indicators would be the best one to use in the titration? i) methyl orange, Ka = 104 ii) bromthymol blue, Ka = 10-7 iii) thymolphthalein, Ka= 10-10 4....
im really confused can anyone tell me if i answered the highlighted question right?? thank you! Equations: pH = -log [H:04] POH --log [OH-] pH + POH = 14 K [H3O+] [OH') - 1x 10-14 Give two methods of determining the pH of a solution 1) pH meter 2) pH paper a) What is the pH of a 0.0012 M NaOH solution? NaOH →Nat +OH show your work [OH - ] - [NnOH] = 0.0012M POH = -log[OH-] - log...