Answer the ff:
1.)
a.) Calculate the pH of a 100 mL sample of water which has 0.1 mL of 1.0 M HCl added.
b.) Calculate the pH of a 100 mL sample of water which has 0.1 mL of 1.0 M NaOH added.
Answer the ff: 1.) a.) Calculate the pH of a 100 mL sample of water which...
Calculate the pH of a 1L solution of water to which is added: 10 ml 5M HCl 10 ml 5M NaOH
Calculate the pH after adding 0.5 mL of 0.1 M HCl to 100 mL of a phosphate buffer in which [H2PO, ] = [HPO? 1=0.35 M? What will be the effect on the initial pH? 3 Part I: Preparation of acetate buffer solution (20 points) Solution Initial pH After adding 2 ml HCI After adding 2 ml NaOH Distilled water 7.1 2.2 12.5 Acetate buffer 4.5 4.3 4.7 Determination of K of the buffer solution Calculated Concentration of CH3COOH Calculated...
a) Calculate the pH of a titration of 100 mL 1.5M HCl with 1.25M NaOH at equivalence. WHY is the pH what it is (if it’s 7, why is the solution neutral? If not 7, why?) b) Calculate the pH of a titration of 100 mL 1.5M HCOOH (Ka = 1.8 x 10-4) when 75 mL 1.25M NaOH has been added. c) What volume of 1.25M NaOH must be added to 100 mL of 1.5M HCOOH to reach equivalence?
Calculate the change in pH when 1.0 mL of 1.00 M HCl is added to 100 mL of a solution of 0.100 M NaCH3COO and 0.100 M CH3COOH.
5. Exactly 100 mL of 0.15 M nitrous acid (HNO2) are titrated with a 0.15 M NaOH solution. Calculate the pH for [10 pts] the point at which 100 mL of the base has been added. 5. Exactly 100 mL of 0.15 M nitrous acid (HNO2) are titrated with a 0.15 M NaOH solution. Calculate the pH for [10 pts] the point at which 100 mL of the base has been added.
Please help, I'm so confused!!!! This is due wednesday night!!! i'm gonna fail :(((( pH of Buffer Solutions Procedure: Acetic Acid-Sodium Acetate Buffer (pKa acetic acid = 4.75) Weigh about 3.5 g of Na2C2H302 3H2O, record the exact mass, and add to a 250 ml beaker. Measure exactly 8.8 mL of 3.0 M acetic acid (use 10 mL grad cylinder) and add to the beaker containing the sodium acetate. • Measure exactly 55.6 mL of distilled water and add to...
Calculate the following: a. The pH of a 500.0 mL buffer solution containing 0.75 M HCN (Ka = 6.2 x 10^-10) and 0.55 M NaCN b. The pH of the above buffer after the addition of 100.0 mL of 1.0 M NaOH. c. The pH of the buffer if 100.0 mL of 1.0 M HCl was added to the solution in part a.
Calculate the pH of the resulting solution if 20.0 mL of 0.200 M HCl(aq) is added to 30.0 mL of 0.200 M NaOH(aq). pH = Calculate the pH of the resulting solution if 20.0 mL of 0.200 M HCl(aq) is added to 10.0 mL of 0.300 M NaOH(aq). pH = Calculate the pH of the resulting solution if 21.0 mL of 0.210 M HCl(aq) is added to 26.0 mL of 0.210 M NaOH(aq). pH = Calculate the pH of the...
Calculate the concentrations of NaOH and maleic acid. 100 mL of 0.1 M NaOH was transferred into a buret. 0.433 g of maleic acid was dissolved in a 100 mL volumetric flask. 25 mL of this solution was transferred into a plastic beaker, and 50 mL of distilled water was added. 6 mL of NaOH was added to get to the first equivalence point (brought pH to 1.99), and a total of 30 mL was added to reach the second...
1. Calculate the equilibrium concentrations of all species present and the pH of a solution obtained by adding 0.100 moles of solid NaOH to 1.00 L of 15.0 M NH3. Kb = 1.8 × 10–5 2. One mole of a weak acid HA was dissolved in 2.0 L of water. After the system had come to equilibrium, the concentration of HA was found to be 0.45 M. Calculate the Ka for this weak acid. 3. Calculate the pH of a...