Procedure: Mix 0.01M KMNO4 and 2 drops of 6M H2SO4 with several drops of 1.0M K2C2O4. Observation: A slight color peach begins to appear.   5K2C2O4(aq) + 2KMnO4(aq)+ 8H2SO4(aq) → 2MnSO4(aq) + 10CO2(aq) + 6K2SO4(aq) + 8H2O(l)   Has oxidation and reduction occurred? If oxidation and reduction has occurred? If oxidation and reduction has occurred define the change in oxidation numbers for the following atoms and define what is undergoing oxidation and reduction:   Mn[ ? ] → Mn[ ? ]   C[ ? ] → C[ ? ]

3) What is the pH of a 0.02 M solution of sodium propionate? (12 pts) Reaction of sodium propionate in water: Pr (aq) + H₂O (1) ⇒ HPr (aq) + OH-(aq) Ka= 10-4.⁹ *Hint* This is a Kb problem therefore you must convert ka to Kb. You can assume that the sodium propionate dissociates completely from the propionate and is not involved in any other important reactions. a) Is this the conjugate base or an acid that you are adding to solution? b) Write down the Mass-Balance Relations, the Proton Balance Relation and the c) Equilibrium Relation. Calculate the pH using both an analytic method, and by drawing the predominance diagram. *Hint* [OH-]=[HPr].

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how do you enter this into a calculator to get 5.8

An analytical chemist is titrating 186.4 mL of a 0.3400M solution of methylamine (CH3NH₂) with a 0.6900M solution of HIO3. The pK² of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 98.0 mL of the HIO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO3 solution added. Round your answer to 2 decimal places. pH = 1 X Ś

Benzoic acid, HC7H5O2, has a Ka value of 6.4 x 10-5. 1. Find the pH of a 1.50 M solution of benzoic acid. 2. Find the pH of a solution made by mixing 600. mL of the benzoic acid solution from part A with 450. mL of a 2.00 M solution of lithium benzoate, LiC7H5O2.  3. Find the pH of a solution made by adding 36.0 grams of sodium hydroxide, NaOH, to the solution created in part B.

pH = 10.31 Use the following table to predict the best acid/ base pair for the desired pH/pOH values below (hint: remember buffer range = ± 1 pKa unit). Acid Base     Name Acid Base pKa Hydrochloric acid HCl Cl- -7.00 Phosphoric acid H3PO4 H2PO4- 2.12 Hydrofluoric acid HF F- 3.18 Lactic acid Lactic acid Lactate 3.85 Acetic acid CH3COOH CH3COO- 4.74 Carbonic acid H2CO3 HCO3- 6.36 Dihydrogen phosphate H2PO4- HPO42- 7.21 Ammonium NH4+ NH3 9.25 Hydrocyanic acid HCN CN- 9.31 Bicarbonate HCO3- CO32- 10.25 Methylammonium ion CH3NH3+ CH3NH2 10.62 Hydrogen phosphate HPO42- PO43- 12.38

A scientist needs to prepare an acetate buffered solution at pH 5.0. What is the final concentration of acetic acid (pKa 4.76) and sodium acetate she needs in the solution to have a create a final concentration of 25 mM? The answers are  [Acetic acid] = 9.12 mM [acetate] = 15.88 mM but I do not know how to get to those answers.

ou need to produce a buffer solution that has a pH of 5.03. You already have a solution that contains 10. mmol (millimoles) of acetic acid. How many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution? The pKa of acetic acid is 4.74.   Express your answer in millimoles.

12:04 Question 4 of 9 Submit A buffer solution contains dissolved C6H5NH2 and C6H;NH;CI. The initial concentration of C6HŞNH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6HŞNH3* in the solution. The value of Kb for C6H;NH2 is 3.8 × 10-1º. 1 2 3 Let x represent the original concentration of C6H,NH,* in the water. Based on the given values, set up the ICE table in order to determine the unknown. C6H5NH2(at H20(1) = OH-(aq) +C6H5NH3*(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.50 - 4.20 -4.20 6.3 x 10-5 -6.3 x 10-5 1.6 x 10-10 -1.6 x 10-10 3.8 x 10-10 -3.8 x 10-10 x + 4.20 x - 4.20 x + 6.3 x 10-5 х - 6.3 х 10-6 x + 1.6 x 10-10 x - 1.6 x 10-10 x + 3.8 x 10-10 x - 3.8 x 10-10 Tap here or pull up for additional resources