Create 50 mL of a pH = 10.00 buffer solution using solid bicarbonate (NaHCO3, baking soda, pKa = 10.30), solid sodium carbonate monohydrate (Na2O3•H2O, washing soda), and distilled water. Use only 1 g of NaHCO3 (record your exact amount), and calculate the mass of Na2O3•H2O needed to create the correct mole ratio.

You are titrating 90.0 mL of a weak base solution (A-) with a concentration of 0.0515 M, using an HCl solution with a concentration of 0.0662 M. Note that the Ka Value for the conjugate acid , HA, is 5.6 x 10-10 . a) What is the pH of the initial weak base solution? b) What is the pH of the solution at the equivalence point? c) What is the pH of the solution when an additional 10 mL of HCl solution is added after reaching the equivalence point?

A student is preparing a buffer at a pH of 8.60. She has these chemicals in the lab: HCl, KOH, H3PO4, KH2PO4, K2HPO4, and K3PO4. Which two chemicals should she use? For H3PO4, pKa1=2.15, pKa2=7.20, pKa3=12.38

The Ka of hydrocyanic acid (HCN) is 4.0 × 10-10.  Determine the pH of a 0.300 mol/L solution of hydrocyanic acid. [3 T]                1. What is the pH at the equivalence point if 25.00 mL of the                 hydrocyanic acid is titrated with 0.300 mol/L NaOH.

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.

8. You will perform some calculations to see the difference between a pH buffer solution and a weak acid solution of the same pH when a small amount of strong base is added. Chlorous acid, HC1O₂, is a moderately strong acid with a Ka = 1.110×10-². Please answer the following questions. A. B. What is the molarity of the HClO₂ solution whose pH is 2.21? Please provider your answer below. 미ㄷ → Please provider your answer below. f A $ To prepare a buffer solution of the same pH, what is the molarity of the NaClO₂ if the molarity of the HC1O₂ is 0.6771 M? M → M → $

Calculate the pH of a buffer solution prepared by dissolving 19.50 g of sodium cyanate NaCNO (65.01g/mol) in 1.00 M  cyanic acid (HCNO) to a final volume of 1.00 liter of solution.    Ka(HCNO) = 3.50 x 10-4

For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 1.0 M NaH2PO4 and 0.50 M Na2HPO4. H2PO4-  + H2O ⇌  HPO42-  + H+         pKa= 7.21 From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis?

You need to prepare a buffer solution from NaH2 PO4 and Naz HPO4 to have a pH of 8.00. What ratio of amounts of Naz HPO4 and NaH2PO4 should you take? (Ka2 = 6.2 × 10-8) (Simplify your answer completely.) n(Naz HPO4) n(NaH2 PO4)

1. Moly Cule is titrating 0.2 M of a strong base (NaOH) into 100 ml of a solution of 0.1M weak acid (HAc).  Ka for HAc is 1.8x10 -5.  What is the initial pH of the solution (before the titrant is added)?