As a technician in a large pharmaceutical research firm, you need to produce 450. mL of 1.00 mol L potassium phosphate buffer solution of pH = 7.03. The pKa of H2PO4 is 7.21. -1 You have the following supplies: 2.00 L of 1.00 mol L-1 KH2PO4 stock solution, 1.50 L of 1.00 mol L- K2HPO4 stock solution, and a carboy of pure distilled H2 O. How much 1.00 mol L- KH2PO4 will you –1 need to make this solution?

Part A As a technician in a large pharmaceutical research firm, you need to produce 450. mL of a potassium dihydrogen phosphate buffer solution of pH = 6.86. The pK of H,PO is 7.21. You have the following supplies: 2.00 L of 1.00 M KH,PO stock solution, 1.50 L of 1.00 M K, HPO stock solution, and a carboy of pure distilled H2O. How much 1.00 M KH,PO will you need to make this solution? (Assume additive volumes.) Express your answer to three significant digits with the appropriate units. Part b

Cacodylic acid (dimethylarsinic acid, HASO2(CH3)2) is a common buffer used in biology to prepare and fix biological samples. The pKa of cacodylic acid is 6.3. Part A What is the pH of a buffer solution prepared by mixing 20.0 mL of 0.0600 mol L-'NaOH with 20.0 mL of 0.105 mol L-!cacodylic acid? Express your answer using one decimal place. femplates Symbols uado redo reset keyboard shortcuts help, pH = Submit Request Answer Part B What is the pH of the buffer solution in part A after 0.0002 moles of H30+ was added to the mixture? Express your answer using one decimal place. Templates Symbols undo redo reset keyboard shortcuts help, pH =

A titration system is set up as follows: the bottom flask contains a sample solution of 50.0-mL 0.50 M C2H3NH2 (ethylamine), the burette is filled with 0.20 M HCl as titrant.   Kb of C2H3NH2 = 6.5 ´ 10-4          What is the initial pH of above sample solution before titration starts?

What is the pH of a buffer solution that is 0.214 M in ammonia and 0.390 M in ammonium chloride (NH4CI)? The Kü of ammonia is 1.8 x 10-5. (Two decimal places)

A TRICINE buffer is made to a pH of 8.15 at 25 °C then warmed to 37 °C. The pH of the solution changes because the pK, changes. TRICINE has a pK, = 8.14 and a ApK/AT= -0.018 "C¹, Calculate the pH of the buffer at 37 °C. pH =

At 22 ˚C, an excess amount of a generic metal hydroxide, M(OH)₂, is mixed with pure water. The resulting equilibrium solution has a pH of 10.20. What is the Ksp of the salt at 22 °C? K sp= APR 9 $ 4 % mtv G Search or type URL 5 MacBook Pro < 6 ONT17 X & 7 = 11 * 00 66 8 + A ( 9 < *** m - ) O W P { + 17 [ = } 1 delete

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Chemistry (Part -3) =============

5:51 1 .ll LTE Search Question 16 of 20 Submit Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH, with 0.100 M HNO3 after 80.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. 1 2 4 Based on the result of the acid-base reaction, set up the unknown. ICE table in order to determine the H2NNH3*(at H2O(1) =H;O*(aq) H2NNH2(aq + Initial (M) Change (M) Equilibrium (M) RESET 0.100 0.200 0.0333 0.0667 +x -X 0.100 + x 0.100 - x 0.200 + x 0.200 - x 0.0333 + x 0.0333 - x 0.0667 + x 0.0667 - x www