NEED help with these questions Question 1 (1 point) Saved The Ksp of PbCl2 is 1.2...
Question 10 1 pts The molar solubility (in M) of PbCl2 in a 0.20 M solution of HCl is This molar solubility is...than the molar solubility of PbCl2 in pure water. The Ksp of PbCl2 is 1.6x10 O 4.0x10-4 M, higher O 4.0x104 M, lower O 80x105 M, higher 8.0 x 10'5 M, lower
What is the Molar Solubility (concentration, M) of PbCl2 in pure water. Remember that its Ksp = 1.17 X 10-5. PbCl2 (aq) = Pb2+ (aq) + 2Cl- (aq) 1.43 X 10-2M 1.21 X 102 M O 7.19 X 10-5M O 1.50 M
PLEASE HELP ME WITH THESE ASAP ! I PLEASE ! Question 15 Select the Ksp expression for the following reaction: Z2XO2 (s) = 2z+ (aq) + XO, 2- о O Knp = [224] (x03-] [x0,2] [3] KA [22X03] O Kg = [Z+] [x0;-) = D Question 16 Calculate the molar solubility of YZ (s) (Ksp - 2.56 x 10-5) in 0.10M Naz (aq). HINT - What is the Common lon? 2.56x10M 0.010M 5.06x100M
please help me 1. a. What is the molar solubility of Ag2SO4 (Ksp = 1.2 x 109) in water? b. How do you expect the solubility to change if the Ag2SO4 were in a 0.10M AgNO3 solution (increase, decrease, stay the same)? Why? C. Calculate the molar solubility of Ag2SO4 in 0.10M AgNO3. d. How do you expect the solubility to change if the Ag2SO4 were in a 0.10M HCl solution (increase, decrease, stay the same)? Why? Your explanation should...
In need of help 1 – List four factors that affect the strength of an acid. All four may not apply to every acid. 2 – Calculate [OH-] for a 1.4 x 10-3 M HCl solution. 3 – Calculate the pH of an aqueous solution at 25 ̊C at is 0.34 M in phenol (Ka = 1.3 x 10-10) .4 – Calculate the concentration at which a monoprotic acid with Ka = 4.5 x 10-5 will be 2.5% ionized. (The...
Can you please try to answer these four questions for me? 3 pts Question 22 20.0mL of a 0.100 M solution of HA is mixed with 10.0mL of water. The pH of the solution is 1.25. What is the Ka of the acid? Report your answer to 3 decimal points. 3 p Question 27 Determine the molar solubility of an ionic compound with the general formula X,Y, where X is the cation and Y is the anion, given a Ksp...
1) Rank the following titrations in order of increasing pH at the halfway point to equivalence (1 = lowest pH and 5 = highest pH). 100.0 mL of 0.100 M KOH by 0.100 M HCl 200.0 mL of 0.100 M HC2H3O2 (Ka = 1.8 x 10-5) by 0.100 M NaOH 100.0 mL of 0.100 M NH3 (Kb = 1.8 x1 0-5) by 0.100 M HCl 100.0 mL of 0.100 M HI by 0.100 M NaOH 100.0 mL of 0.100 M...
1.) Rank the following titrations in order of increasing pH at the halfway point to equivalence (1 = lowest pH and 5 = highest pH). 100.0 mL of 0.100 M C2H5NH2 (Kb = 5.6 x 10-4) by 0.100 M HCl 200.0 mL of 0.100 M HC2H3O2 (Ka = 1.8 x 10-5) by 0.100 M NaOH 100.0 mL of 0.100 M HF (Ka = 7.2 x 10-4) by 0.100 M NaOH 100.0 mL of 0.100 M HCl by 0.100 M NaOH...
need help with all parts of question 2. thank you :) equivalence points and the pH at the half equivalence points for the three titration regions. Question 2 Part A Given the Ksp = 2.0 x 10-29 for the sparingly soluble salt, calcium phosphate (Ca3(PO4)2), determine the molar solubility of the salt in a solution that is 0.20 M in calcium perchlorate, Ca(C104)2. Part B The cation, Co2+, is able to form a complex ion, (Co(SCN)4] 2-, with the thiocyanate...
Please explain the correct answer for both questions. Thank you! Incorrect Question 7 0/1 pts The concentration of iodide ions in a saturated solution of lead (11) iodide is_ The solubility product constant of Pblz is 1.4x10-8. 3.5x10-9 3.0x10-3 1.5x103 1.4x10-8 3.8x10-4 Incorrect Question 9 0/1 pts The molar solubility of lead () chloride (PbCl2) is 1.6x102 M. What is the Ksp of PbCl2? 4.1x10-6 5.0x10-4 1.6x10-2 3.1x107 1.6x10-5