4. Calculate the pH and percent dissociation of the solution when 125.0 mL of 0.100 M...
i need help with number 4 and 5 please 4. How many mL of 0.100 M NaOH should be added to 500.0 mL of 0.150M acetic acid to produce a buffer pH 4.0? pKa acetic acid 4.757. ANSWER: 112 mL 5. How many mL of 0.100 M HCI should be added to 500.0 mL of 0.150 M sodium acetate to produce a buffer pH 5.0? pKa acetic acid 4.757 ANSWER: 273 mL
Calculate the change in pH when 3.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). NH3 Kb=1.8x10^-5 Calculate the change in pH when 3.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.
Help: what is the pH after mixing If 50.0 mL of 0.100 M NaOH(a) is added to this buffer solutn then what is the final pH? Situation: Consider a buffer system / solution composed of 100.0 mL 0.100 M hydrochloric acid mixed with 300.0 mL of 0.150 M sodium acetate at 298 K.
Question Completion Status: QUESTION 8 What is the percent dissociation of acetic acid if the solution has a pH = 4.74 and a pka 4.74? O 100% O 50% O 10% O 1% QUESTION 9 Consider the titration of 10.00 mL of 0.100 M HCI with 0.150 M KOH at 25°C. What would be the pH of the solution when 10.00 mL of KOH have been added? 1.301 12.699 1.602 12.398 7.000
Calculate the change in pH when 3.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3 (aq) and 0.100 M in NH4CI(aq). Consult the table of ionization constants as needed ДрН Calculate the change in pH when 3.00 mL of 0.100 M N2OH is added to the original buffer solution. АрН -
can someone help me with these two questions? A 15.3 mL solution of 0.100 mol L-1 NaOH is titrated using 0.150 mol L-1 HCI. What is the pH of the solution after 16.7 mL of the HCl solution is added? Express your answer to 2 decimal places. You have 5 attempts at this question. Remember you can find KA and/or KB values in your textbook in chapter 15. Answer: Check A 15.2 mL solution of 0.100 mol L-1 HE is...
Calculate the pH of a mixture when 48.00 mL of 0.100 M NaOH solution is added to 50.00 mL of 0.100 M HCl solution? Write the correct answer in 3 significant figures.
Calculate the pH at the equivalence point when 12.35 mL of a 0.100 M Codeine solution (Kb = 1.6X) is titrated with 0.100 M hydrochloric acid.
Calculate the pH at the equivalence point when 12.35 mL of a 0.100 M Codeine solution (Kb = 1.6X10-6) is titrated with 0.100 M hydrochloric acid.
Ka * Kb = Kw = 1.0 X 10-14 A 25.0 ml sample of a 0.100 M solution of aqueo us ammonia is titrated with a 0.125 M solution of HCI. Calculate the pH of the solution after 0.00, 10.0, 20.0, 30.00, and 40.0 mL of acid have been added; Kb of NH3= 1.8 X 10-5 at 25 °C. Hint: First find the moles after each 10.00 ml of acid is added. Then find the concentration after equilibrium is reached.