NiCO3 + HCl
NiCl2 + CO2 + H2O
Due to odd ion effect the equilibrium will shift in the forward direction hence we can say that sopubility will increases
Option b is correct :- Solubility will increases
Question 31 3 pts How is the solubility of a saturated solution of nickel carbonate, Nico;...
The molar solubility of nickel(II) carbonate in a 0.289 M potassium carbonate solution is ________ M
The molar solubility of nickel(II) carbonate in a 0.170 M sodium carbonate solution is M. Submit Answer Try Another Version 3 item attempts remaining
Part A A student measures the OH- concentration in a saturated aqueous solution of nickel(II) hydroxide to be 8.44×10-6 M. Based on her data, the solubility product constant for nickel(II) hydroxide is Part B A student measures the Pb2+ concentration in a saturated aqueous solution of lead bromide to be 1.14×10-2 M. Based on her data, the solubility product constant for lead bromide is Part C A student measures the molar solubility of silver carbonate in a water solution to...
1. How is the molar solubility of a slightly soluble salt affected by the addition of an ion common to the salt equilibrium? 2. A 3.11 mL volume of a standardized 0.0025 M HCl solution titrated 25.0 mL of a saturated Mg(OH)2 solution to the methyl orange endpoint. Calculate the Ksp of Mg(OH)2. 3. If the endpoint in the titration of a saturated Ca(OH)2 solution with a standardized HCI solution is surpassed, will the reported Kap of Ca(OH)2 be reported...
3 pts Question 2 The chemical equation for calcium oxide and calcium carbonate equilibrium is described below. CaO + CO3(x)= CaCO3(9) AH° = -176 Predict how the following changes would shift the equilibria. Be sure to start by writing the equilibrium (K) equation Increased carbon dioxide concentration Choose ] equilibrium will shift to the left equilibrium will shift to the right equilibrium will be unaffected Increased partial pressure of carbon dioxic [Choose) One half of the calcium carbonate is removed...
Question 4 07 1.5 pts What is the concentration of Pb2+ in a saturated solution of PbCl2 in 0.10 M KCl solution. (Ksp = 1.4 x 108)? Why is [Pb2') in this question (smaller/larger) than in Question 3? Hint: What is the initial [CI] before PbCl2 is dissolved? because the presence of chloride ion prevents the dissolution 1.4 x 10M of PbCl2 1.5 x 10M same as in Question 3 1.4 x 10-M, because the presence of chloride ion slows...
5. (36 pts total) To determine the molar solubility and solubility product constant of magnesium carbonate, Matt stirred 5 g of MgCO3 powder in 150 mL of 0.0041 M MgCl2 solution for 15 minutes. After waiting an additional 10 minutes, he separated the undissolved solid by filtration and collected the filtrate in a dry Erlenmeyer flask. He determined the concentration of CO2 in the filtrate to be 1.40 x 10M Answer the following questions based on Matt's experimental data. For...
Calculating the Effect of a Common Ion on Solubility Consider a saturated solution of the salt MX3, which M is a metal cation with a 3+ charge and X is an anion with a 1− charge, in water at 298 K. Which of the following will affect the Ksp of MX3 in water? Consider a saturated solution of the salt , which is a metal cation with a charge and is an anion with a charge, in water at 298 . Which of the...
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
Part A and Part B.
Also question #3-post lab. (its circled)
A. Molar Solubility and Solubility Product of Calcium Hydroxide Trial I Trial 3 Trial 2 25.0 1. Volume of saturated Ca(OH), solution (mL) 2. Concentration of standardized HCl solution (molU/L) 3. Buret reading, initial (mL 4. Buret reading, final (mL) 5. Volume of HCI added (mL) 6. Moles of HCI added (mol) 7. Moles of OH" in saturated solution (mol) 8. (OH1, equilibrium (mol/L) 9. (Ca2 ], equilibrium (mol/L)...