(15 pts) The pH at the equivalence point where 100.0 mL of 0.53 M NaHCOs is titrated with 0.30 M NaOH solution is 11.77. Ka = 1.5-1013 3. Determine the Ka for НСОЗТ О \ ㄴ (onguns! \) : Ooss.nl 3-5

Calculate the pH at the second stoichiometric point when 425 mL of 0.046 M solution of tartaric acid (Ka1 = 9.2E-4, Ka2 = 4.3E-5) is titrated with 1.00 M NaOH. a. The most suitable indicator for this titration would have pKIn closest to what value?

Please Calculate the mass of sodium acetate trihydrate (CH3COONa●3H2O) solid and thevolume of 1.00 M acetic acid (CH3COOH) required to make 250.0 mL of 0.100 M buffer, pH 5.00 Thank you!

If 21.6 mL of 0.107 M acid with a pKa of 5.16 is titrated with 0.105 M NaOH solution, what is the pH of the titration mixture at halfway to the equivalence point?

How many moles of BHCl (acidic salt) would need to be added to 417 mL of 1.33 M B (a weak base) to produce a solution with a pH equal to 8.99? Report your answer to the thousandths place. The Kb of the weak base (B) is 3 × 10-7

It is necessary to prepare 0.100 liters of buffer pH 4.70 with a concentration of 0.250 M, from a solution of acetic acid at 55.0% m/m (density = 1.010 g/mL) and sodium acetate of purity 97.0 %, how many g of salt do I need? (Ka = 1.78 x 10-5) (Note significant figures).

Suppose you have just added 50.0 ml of a solution containing 0.0400 moles of weak acid HA to 500.0 ml of 0.6000 M NaOH. What is the final pH? The Ka of HA is 1.77 × 10-5.

Show how to prepare a 100-mL phosphate buffer solution (0.1 M, pH 7.0) using 14.8-M concentrated H3PO4 and solids NaH2PO4 ∙ 2H2O, anhydrous Na2HPO4, and anhydrous Na3PO4. Please also include the corresponding equilibrium equation.

5. How would you prepare a liter of “carbonate buffer” at a pH of 10.10? H2CO3 ↔ H+ + HCO3-      Ka = 4.2 x 10-7 HCO3-↔ H+ + CO3-2        Ka = 4.8 x 10-11   a 1stbuffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a 1-L solution   b 2ndbuffer is preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-L solution   c 1stbuffer preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-L solution   d 2nd  buffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a 1-L solution

How many grams of NaF (41.99 g/mol) would need to be added to 465 mL of 0.071 M HF(aq) to produce a solution with a pH equal to 4.47? Report your answer to the thousandths place. The Ka of HF is 6.6 × 10-4.