When excess solid Mg(OH)2 is shaken with 1.00 L of 1.0 M NH,Cl solution, the resulting saturated solution has pH = 9.00. Calculate the Kp of Mg(OH)2.

Q: Calculate the solubility of Mn(OH)2 in grams per literwhen buffered at pH (a) 7.0, (b) 9.5, (c)…

A:

Q: Calculate the molar solubility of CaF2 in a solution containing 0.250 M Ca(NO3)2.

A:

Q: What mass of AgBr will dissolve in 500.0 mL of 5.10 M NH₃? Ksp for AgBr is 5.0 × 10⁻¹³. For the…

A: The given formation reaction is, AgBr ionizes to give Ag+ and Br- Overall reaction is,

Q: 4. Calculate the mass of sodium acetate that must be added to 1.50 L of a 0.456 M acetic acid (Ka =…

A:

Q: 3) What is the solubility of AgCl if the Kp is 1.6 x 10 -10?

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: 130 mL of 0.7 M solution NaHCO3 is titrated by 0.5 M HCIO3 (Kp = 2.4 x 108). (i) What is the pH…

A:

Q: Choose standard substance for standardization of titrant for argentometric titration: NaCl; Na,S2O;;…

A: Ans Standardization  of titrant for argentometric titration( silver nitrate) AgNO3.  Silver Nitrate…

Q: Calculate the molar solubility of AgBr in 0.035 M NaBr (ksp = 5 x 10-13).

A: First the Ksp equation is noted.

Q: Calculate the solubility of Ag Cl (s) in pure water.

A: solubility is defined as the maximum amount of solute that can be dissolve in a solvent or we can…

Q: Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH (a) 11.8

A: Introduction :  We have to calculate Solubility in grams per liter . Given :  pH = 11.8  From this…

Q: Consider Al(OH)3(s) + 3H+(aq) ↔ Al 3+(aq) + 3 H2O(l) a. Calculate K for this reaction. b. Calculate…

A: Given data :  pH of acid = 4.0  a)To get the K value we will devide concentration of products to the…

Q: Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH (a) 7.0 ?

A:

Q: Calculate the solubility of CaC2O4 in a solution containing 0.001 molarity H+

A: Solubility indicates the maximum amount of a substance that can be dissolved in a solvent at a given…

Q: Calculate the molar solubility of AgBr in 0.035 M NaBr (Ksp = 5 × 10–13).

A: AgBr (s) -------> Ag+1(aq)   +  Br-1 (aq)   Ksp = [Br-1] [Ag+1]    AgBr is in NaBr…

Q: Determine the pH of a buffer solution containing 0.150 M of NH3 and 1.2OM of NH&CI. K of NH3 = 1.8 x…

A: Buffer :-  A solution which resists the change in its pH value when small amount of strong acid or…

Q: gravimetric analysis

A: In gravimetric analysis we add a Precipitating reagent into the analyte to make ppt then filter dry…

Q: What is the minimum concentration of OH required to precipitate Cu(OH), in this solution? \- b. What…

A: The Solubility Product (Ksp)  for  Cu(OH)2=[Cu2+][OH−]2 -----------1 Now, given that [Cu2+]= 1 x…

Q: Compare the molar solubility of Mg(OH)2 in pure water with that in a solution buffered at pH 9.00.

A: The dissociation of Mg(OH)2 is Mg(OH)2 s⇋Mg2+ aq+ 2OH- aq. For pure water: Ksp = (s)(2s)2 =…

Q: Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH=9.7.

A:

Q: A buffer consists of 0.21 M H3PO4 and 0.38 M NaH2PO4. Given that the K values for H3PO4 are, Ka1 =…

A: Given that, a buffer is made by 0.21 M of H3PO4 and 0.38 M of NaH2PO4. The dissociation constant…

Q: A buffer solution is made that is 0.482 M in HS and 0.482 M in NaHS. If Ka for H2S is 1.00 x 10-7,…

A: Given: Concentration of weak acid H2S = 0.482 M Concentration of conjugate base salt of weak acid…

Q: A buffer solution is made that is 0.333 M in HNO2   and 0.333 M in NaNO2. If Ka for HNO2 is 4.50 x…

A: Since the solution is having weak monoprotic acid HNO2 and its conjugate base NaNO2  hence the…

Q: What is the maximum concentration of Ag⁺ that can be added to a 0.00300 M solution of Na₂CO₃ before…

A:

Q: 0.0 mL sample of 0.100 M ammonium chloride (NH₂, K, 5.70 x 10 10) is titrated with 0.100 M NaOH.…

A:

Q: - If a 1.0 M solution of NaOH is slowly titrated (dripped) into a 0.050 M solution of Mn2 (aq), what…

A: Given : Concentration of Mn2+ = 0.050 M  And pH of solution becomes 8.00  Since pH = 14 + log[OH- ]…

Q: When K2(S) is added to a saturated solution of FeS , what happens to the solubility of FeS

A: We have to predict about solubility of potassium sulfide.

Q: Calculate the solubility at 25 °C of PbCrO4 in pure water and in a 0.0020 M Na2CrO4 solution.

A: The solubility product, Ksp of PbCrO4 is 2.3 X 10-13  And the solubility reaction with the…

Q: Calculate the solubility in g/100 mL of the AgI in 0.10 M NH3 . The NH3 concentration is that of…

A:

Q: buffer solution is made that is 0.485 M in HNO2 and 0.485 M in NaNO2 . If  Ka for HNO2 is 4.50 x…

A:

Q: Calculate the concentration of PO4^3- when Ag3PO4 starts to precipitate from a solution that is…

A: The solubility product Ksp for Ag3PO4 = 1.8 x 10-18 Ksp expression for the Ag3PO4 , Ksp = [Ag+]3…

Q: The formation constant* of [M(CN)4]2− is 7.70×1016, where M is a generic metal. A 0.130 mole…

A: Assuming M(NO3)2 is completely soluble => moles of M2+ in solution = 0.13 = moles of M(NO3)2…

Q: 3- Calculate the concentration of PO4 when Ag3PO4 starts to precipitate from a solution that is…

A: Answer: Silver phosphate is a sparingly soluble salt, therefore it can be considered that all of its…

Q: Write a balanced net ionic equation to show why the solubility of Mg(OH)2(s) increases in the…

A: Here, let's take the strong acid as conc. HCl.  The reaction is: Mg(OH) 2 (s) + 2HCl (aq) MgCl2 (aq)…

Q: What is the pH of a buffer made from 0.220 mol of HCNO (Ka = 3.5 × 104) and 0.410 mol of NaCNO in…

A:

Q: Determine the molar solubility of AgCl in a 1.0 M solution of NH3. Kp of AgCI - 1.ó x 10 10 K of…

A: Given, Concentration of NH3 = 1M Ksp of AgCl is =1.6× 10^ -10. Kf of Ag(NH3)2 + = 1.5 × 10^7. We…

Q: Calcium hydroxide (Ca(OH)a) is a strong base. Its solubility is about 0.74 g/L at 25°C. 1. For a…

A:

Q: Calculate the molar solubility of Ni(OH)2 when buffered at pH 12.0

A: To calculate the molar solubility of Ni(OH)2 when pH 12.0. The solubility product of Ni(OH)2 is…

Q: A buffer solution is created containing 3.25 M acetic acid and 0.550 M sodium acetate. The Ka of…

A: Given :-  [CH3COOH] = 3.25 M  [CH3COONa] = 0.550 M  Ka for acetic acid = 1.77 x 10-5  To calculate…

Q: Calculate the molar solubility of Ca(IO₃)₂ in (a) 0.060 M Ca(NO₃)₂ and (b) 0.060 M NaIO₃

A: Introduction: Solubility: It is defined as the maximum amount of solute that can be dissolved in the…

Q: Calculate the molar solubility of Ga(OH); (Kp= 7.28 x 10-3) in a solution that is buffered at…

A: Molar solubility of a compound denotes the number of moles of solute which can be dissolved per…

Q: Calculate the pH at the equivalence point for the titration of 0.110 M methylamine (CH,NH, ) with…

A: We need to find pH at equivalence point.

Q: Calculate the K sp for hydroxide if the solubility of Sr(OH) 2 in pure water is 1.42 × 10 1 g/L.

A: Ksp of hydroxide can be calculated as follows

Q: What mass of AgBr will dissolve in 500.0 mL of 1.35 M NH₃? Ksp for AgBr is 5.0 × 10⁻¹³. For the…

A: The two equations as per the question along with their rate constants are given below:- Ag+(aq)    +…

Q: molar solubility

A:

Q: What mass of AgBr will dissolve in 500.0 mL of 5.90 M NH₃? Ksp for AgBr is 5.0 × 10⁻¹³. For the…

A: The overall reaction for the solubility of AgBr in ammonia can be written as follows:

Q: Consider the titration of 15.75 mL of 0.549 M potassium propanoate, CH3CH;CO,K, with 0.207 M HNO3.…

A: Given : Concentration of CH3CH2CO2K = 0.549 M Volume of CH3CH2CO2K solution = 15.75 mL = 0.01575 L…

Q: Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH (a) 12.5

A: pH = 12.5 pOH =14 -12.5=1.5