Calculate the molar solubility of BaCO3in a 0.10 M solution of Na2CO3(aq). (Ksp(BaCO3) = 8.1 x 10-9)

Q: The solubility of Pb3(AsO4)2 is 3.0 x 10-5 g/L. What is the solubility product constant?

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Q: Iron(II) hydroxide, Fe(OH)2, has a solubility in water of 6.0 x 10¹ mg/L at a given temperature. (a)…

A: Solubility product is defined as the product of the concentration of the ions which is in…

Q: The pH of a 0.30 M NH3 / 0.36 M NH4Cl buffer solution is 9, 17. what is the pH after the addition of…

A: Step 1: Given[NH3] = 0.30 M[NH4Cl] = [NH4+] = 0.36 MVolume of buffer = 80 mL = 0.080 LpH = 9.17pKb =…

Q: Will Mn(OH)2 precipitate from solution if the pH of a 0.050 M solution of MnCl2 is adjusted to 8.0?…

A: Solubilty product of Mn(OH)2 is, ksp = 2 × 10-13Solubilty product of Ag2SO4 is, ksp = 1.5 × 10-5…

Q: Consider the titration of 300.0 mL of 0.450 M NH3 (Kb = 1.8  10–5) with 0.450 M HNO3. At the…

A: pH of an aqueous solution of a salt of a weak base and strong acid = 7 - (pKb + logC)/2 Where, pKb =…

Q: You have 30.00 mL of a 0.250 M aqueous solution of the weak base (CH3)2NH (Kb= 7.40 x 10-4). This…

A: Given,  Molarity of weak base, (CH3)2NH = 0.250 M  Volume of (CH3)2NH = 30.00 mL  Base dissociation…

Q: 2a) Does a precipitate form when you add 55.5 g of NaCl to 250.0 mL of 0.35 M Pb(NO3)2?  (Ksp for…

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Q: The pKa of a weak acid acid HA is 4.47. Consider the titration of 100 mL of 200 mM HA (aq.) with 200…

A: Weak acid is a an acid that does not dissociates completely in solution rather maintains an…

Q: A mixture of 20.0ml of 0.10M Ba(NO3)2 with 50.0ml of 0.10M Na2CO3. what is the cation concentration…

A: Certain solid compounds formed in precipitation reactions do not dissociate completely in solution.…

Q: The Ksp for BaCO3 is 5.1×10−9.5.1×10−9.  How many grams of  BaCO3 will dissolve in 1000. mL of…

A: Answer: 1000mL is equal to 1 Liter, therefore first of all we will find out the solubility in mol/L…

Q: What is the solubility of NH3 if its partial pressure is reduced to 30,000 Pa?

A: According to Henry’s law, the solubility of a gas is expressed as S = KP where S is the solubility,…

Q: Consider the reaction of a 20.0 mL of 0.220 M C5H5NHCI (Ka = 5.9 x 10-6) with 12.0 mL of 0.241 M…

A: At the start of the titration, moles of C5H5NHCl are equal to C5H5NH+. Given molarity of C5H5NHCl is…

Q: What is the pH of a buffer solution made of .50 M CH3CO2H and .36 M NaCH3CO2? pka= 4.7 for CH3CO2H

A: Step : 1         What is the pH of a buffer solution made of .50 M CH3CO2H and .36 M NaCH3CO2? pka=…

Q: The solubility-product constant for Ce(IO3)3 is 3.2 X 10-10. What is the Ce3+ concentration in a…

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Q: A buffer consists of 0.50 M NaH₂PO₄ and 0.40 M Na₂HPO₄.Phosphoric acid is a triprotic acid…

A: A buffer solution is prepared by mixing a weak acid and its conjugate base in the aqueous medium.…

Q: Consider a buffer made by adding 132.8 g of NaC7H5O₂ to 300.0 mL of 1.83 M HC7H5O₂ (Ka = 6.3 x 10-5)…

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Q: 1. Calculate the solubility in mg/L at 25 °C in the presence of 0.010 M CaCl2. Neglect other…

A: At 25°C Ca3C6H5O72 has a Ksp of 1.12 × 10-15 . We have to calculate the solubilility of calcium…

Q: A chemistry graduate student is given 450. mL of a 0.90 M propanoic acid (HC,H,Co, solution.…

A: Answer :-  Henderson-Hasselbalch equation is used to determine the PH  of a buffer solution. The…

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for