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Which of the following salts would be an insoluble product? *Select all that apply!*
NaCl
BaSO4
AgCl
K3PO4
CuNO3
SrS
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- What weight of PbCl2 will dissolve in 200 mL of 0.25 M NaCl solution?A solution is 0.020Min Mg2+(aq)and 0.20Min Ni2+(aq). Ksp(Mg(OH)2) = 8.9x 10-12; Ksp(Ni(OH)2) = 1.6x 10-16. b.Calculate the maximum concentration of hydroxide ionto precipitate only one compoundPLEASE SHOW SOLUTIONS QUESTION NO. 1: A 0.097 N silver nitrate solution of 56.3 ml was used to titrate two samples of sodium lauryl sulfate with 3g and 5g, each respectively. Calculate the %NaCl in the sample, then interpret. Please answer very soon will give rating surely
- From the value of Kf listed in Table, calculate the concentrationof Ni2+ (aq) and Ni(NH3)62+ that are present atequilibrium after dissolving 1.25 g NiCl2 in 100.0 mL of0.20 M NH3(aq).For ammonia, Kb is 1.8 × 10–5 . To make a buffered solution with pH 10.0, the ratio of NH4Cl to NH3 must be Question 27 options: A) 1.8 : 1. B) 0.18 : 1. C) 1 : 1.8. D) 1 : 0.18. E) none of theseBuffer Capacity and pH Change1. Calculate the pH of the solution containing 0.20 M ammonia and 0.30 M ammoniumchloride. Calculate the pH change if 100 mL of, (a) 0.05 M hydrochloric acid (b) 0.05 Msodium hydroxide, is added to 400 mL of the buffer.
- Please answer it ALL ASAP and CORRECTLY for an upvote. PROVIDE YOUR FULL SOLUTION. You prepared a buffer solution by mixing 68 ml of 0.17 M ammonia and 42 ml of 0.13 M ammonium chloride. The dissociation constant of ammonia is 1.8x10^-5 What is the total volume of the buffer? What is the final concentration of the base? What is the final concentration of the salt? What is the acid strength of the solution? What is the pH of the buffer solution?Indicate your predictions beneath the reaction (using one the following symbols →, ←, ↓, ↑ where appropriate) following the application of stress to the equilibrium reactions: On treatment with 6 M NaOH which direction will the equilibrium adjust to minimize the “stress” Shift left (←) or right (→)? Fe3+ (aq) SCN- (aq) <-> [Fe(SCN)]2+(aq) What is the function of the vacuum aspirator? Predict the color shift of the indicator as a consequence of the applied “stress”. Originally greenish-yellow because of 1M of HCL added. HCO3-(aq) <-> CO2(g) + OH- (aq)a)What would the balanced equation be in a basic solution? Show all your steps. b) What would the color change of the solution be at the equivalence point? Why? c) If you were to over-titrate, explain whether your calculation for % FeCl2 would be too high or too low and why.
- The pH of a buffer solution containing 0.5 mole/litre of CH3COOH and 0.5 mole/litre CH3COONa has been found to be 4.76. What will be the pH of this solution after 0.1 mole/litre HCl has been added to the buffer? Assume that the volume is unchanged. Ka = 1.75 × 10– 5How will the reported solubility product of borax be affected if the solid borax is contaminated with NaCl?d) please see attached question concentration KOH=20.8325mL pH solution=2.9 beginning of the titration, Vbase = 0.00 mL
