Determine either Ka or Kb for the following salts. Initial concentration of salts are 0.1M.
pH= 9.1
NaC2H3O2
Determine either Ka or Kb for the following salts. Initial concentration of salts are 0.1M. pH=...
Determine the pH of each of the following solutions. Ka acetic acid is 1.8*10^-5. Kb ammonia is 1.76*10^-5 Part A. 0.20 M NH4Cl Part B. 0.19 M NaC2H3O2 Part C. 0.12 M NaCl Thank you!
EXPT 5 HYDROLYSIS OF SALTS Use Ph to calulate H+ and OH- SOLUTION Measured pH Calculated [H+] Calculated [OH-] H2O(boiled) 7 0.1M NaCl 7 0.1M Na2CO3 13 0.1M NaC2H3O2 8.8 0.1M NH4Cl 4.6 0.1M Al(NO3)3 4 0.1M ZnCl2 5 0.1M KAl(SO4)2 4
Determine Ka and Kb for 0.10M NH3 with a pH of 11.12.
- Given this concentration n ratio what is the pH (show work), Ka and percent ionization of this species ( HA+H2O← → A- + H3O+ , acid. Initial concentration: 0.01 mol/L) HA: 9.77x10^-3 mol/L H2O: 55.6 mol/L A- : 2.34x10^-4 mol/L H3O+: 2.34x10^-4 mol/L - Also if we increase the initial concentration how does this affect the ph n the Ka such as increasing it to .1mol/L - is you have initial concentration of .001 if u increase strength what...
Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 times 10-5. Determine the [OH-] concentration in a 0.169 M Ca(OH)2 solution. Determine the pH of a 0.227 M C5H5N solution at 25 Degree C. The Kb of C5H5N is 1.7 times 10-9 Determine the Ka for CH3NH3+ at 25 Degree C. The Kb for CH3NH2 is 4.4 times 10-4.
Part B: Using Ka or Kb 4. What is the pH for an acid that is 1.5 M and K. - 3.2 * 10-5? 5. What is the pH for a base if the concentration is 0.0045 M and Kb - 2.3 - 10-72 6. What is the pH of 0.59 M NaNO2 if the K, for HNO2 is 7.1*10-4?
1) Determine the pH of a 0.0785 M unknown weak base solution. Kb of the unknown weak base is 4.7 x 10−6. 2) An unknown weak acid solution with a concentration of 0.0850 M has a pH of 4.35. What is the Ka for this weak acid? 3) What is the pH of a 0.0380 M solution of HNO2? (Use your workbook to find Ka) 4) An unknown weak base solution with a concentration of 0.187 M has a pH...
Equations pH=-log[H3O+]; pOH= -log[OH]; pKw=14.00=pH+POH; Ka-[H3O+][A-[HA]; Kb=[BH+][OH-)[B); pKa=-log Ka; Ka. Kb=Kw Constants Ka (HS-)=1x10-19; Ka (HF) 7.2x10-4; Ka ([Al(H20).]+)7.9x10-6; Ka (H3PO4)=7.5x10-2: Ka (HPO42-) =3.6x10-13; Ka (HCI)=Huge; Ka(Na+)=tiny; Ka(Cl-)tiny; Kb(NH3)=1.8x10-5; Kw=1x10-14 1) Calculate the pH of aqueous 0.25M HCl and 0.25M HF solutions. 2) Complete the following tables for aqueous solutions of conjugate acid-base pKa pKb Kb 1.3x10-4 35 3) Complete the following table for aqueous solutions DHL TH+) OH) pOH 1x102 4) Calculate the pH of aqueous 0.15M Ba(OH)2 and...
Please show all your work for the problems! Exp Composition Total Vol pH 1 A few mL of 0.10M NH3 (unchanged) n/a 11.13 2 2.5mL 0.1M NH3 & 7.5mL H2O 10 ml 10.82 3 2.5mL 0.1M NH4Cl & 7.5mL H2O 10 ml 6.01 4 2.5mL 0.1M NH3 & 2.5mL 0.1M NH4Cl & 5mL H2O 10 ml 9.26 5 Take 1mL Solution #4 and add 9mL of water 10 ml 9.26 Solution 1. Use the concentration of NH3 and the measured...
use a table of ka and kb to determine pH of the 0.10 M CH3NH3Cl d. 0.10 M CHÁNH,CI 4. Use the table of K and K values to predict whether a solution of NH CN is acidic, basic, or neutral. Explain your choice.