Q: The solubility of PbI2 is 1.3 x 10–3 mol*L–1.What is the Ksp for PbI2?
A: Given S = 1.3 x 10-3 mol L-1
Q: What is the solubility of Mg(OH)₂ at a pH of 12.40? (Ksp Mg(OH)₂ is 1.6 × 10⁻¹³)
A: Concentration of OH- is calculated as follows, pH+pOH=14.Thus,pOH=14 -pHpOH=14…
Q: What is the solubility of Mg(OH)2 at a pH of 12.40? (Ksp Mg(OH)2 is 1.6 × 10¯13)
A:
Q: The molar solubility of the metc hydroxide (M(OH)2) in water is: M(OH)2 = M2+ + 20H Ksp = 5.02 x…
A: Given, Ksp = 5.02 x 10-6 Molar solubility , S = ?
Q: What is the solubility of Mg(OH)₂ at a pH of 12.10? (Ksp Mg(OH)₂ is 1.6 × 10⁻¹³)
A:
Q: What is the solubility of La(IO₃)₃ in a solution that contains 0.100 M IO₃⁻ ions? (Ksp of La(IO₃)₃…
A:
Q: What is the solubility of MgCO3 in a solution that contains 0.050 M Mg2 ions? (Ksp of MgCOs is 3.5 x…
A:
Q: For calcium fluoride, CaF2, Ksp = 4.0 x 10-11. What is the minimum concentration of Ca2+needed to…
A: Given: CaF2
Q: For Cu(OH)2, Ksp = 1.6 x 10-1⁹. What is the molar solubility of Cu(OH)2?? 5.1 x 10-10 M 3.4 x 10-7 M
A: Molar solubility of Cu(OH)2 can be calculated from its solubility product expression.
Q: What is the solubility of barium sulfate in a solution containing 0.050 M sodium sulfate? The Ksp…
A: the solubility of barium sulfate in a solution containing 0.050 M sodium sulfate. Here common ion…
Q: What is the solubility of MgCO₃ in a solution that contains 0.075 M Mg²⁺ ions? (Ksp of MgCO₃ is 3.5…
A: In this question, we want to calculate the Solubility of MgCO3 How we can calculate, you can see…
Q: What is the solubility of Mg(OH)₂ at a pH of 12.70? (Ksp Mg(OH)₂ is 1.6 × 10⁻¹³)
A: Magnesium hydroxide dissociates in solution to give the following ions, Mg(OH)2→Mg2+(aq)+2OH-(aq)
Q: What is the solubility of PBF2 in a solution that contains 0.0400 M Pb2* ions? (Ksp of PbF2 is 3.60…
A: PbF2↔ Pb+2+F-let initial concentration of Pb+2=x , F-=2x Mwhen , PbF2 added to a solution , that…
Q: What is the solubility of Mg(OH), at a pH of 12.70? (Ksp Mg(OH)2 is 1.6 x 10-13)
A: Given, pH = 12.70 We know that, pH + pOH = 14 => pOH = 14-pH…
Q: The solubility of FeF2 in pure water at 25°C is 0.0133 M. What is the solubility of FeF2 in a…
A: Answer:- Firstly a balanced dissolution equation is written then using the molar molar solubility,…
Q: Calculate the solubility (in M) of cobalt(I) hydroxide, Co(OH)2(s) in H2O. Ksp = 2.70x10-16 at a…
A:
Q: What is the molar solubility of CaF2 in a solution containing 0.050 M Ca(NO3)2? (Ksp for CaF2 is 3.9…
A: Solubility of CaF2 can be calculated by first writing Solubility product expression and then solving…
Q: The Ksp of CaSO4 is 2.4x10-5. What is the molar solubility of CaSO4 in 0.11 M aqueous Ca(NO3)2?
A: All known compounds can be dissolve in certain solvents whereas they remain insoluble in other…
Q: What is the minimum mass of Mg(NO3)2 that must be added to 1.00L of a 0.760 M HF solution to begin…
A: Let us solve this question step by step.
Q: What is the solubility of MgCO₃ in a solution that contains 0.065 M Mg²⁺ ions? (Ksp of MgCO₃ is 3.5…
A: This is a portion of common Ion solubility so use concept of solving this question. higher power of…
Q: The solubility of Gd2(SO4)3 is 4.0 g/100 mL. What is the Ksp?
A:
Q: The solubility product for chromium(III) fluoride is Ksp = 6.60 X 10-11. What is the molar…
A: Given, Solubility product of chromium(III) fluoride = 6.60*10-11. The reaction of chromium(III)…
Q: The Ksp of calcium fluoride is 3.9 × 10-11. Calculate the concentrations of calcium and fluoride…
A: The value of solubility product of CaF2 is 3.9×10-11. The dissociation of CaF2 in aqueous solution…
Q: The value of Kep for PbCroa (s) in equilibrium with water at 25 °C is 2.8 x 10-13, Calculate the…
A: Answer :- The Solubility of PbCrO4 in water at 25 °C in g/L = 1.7 × 10-4 (g/L)…
Q: Solid PbI2 (Ksp=9.8x10-9) is placed in a beaker of water. After a period of time the lead(II)…
A: Solubility product is a equilibrium constant for a solid substance. Mathematically it is the…
Q: What is the solubility of Mg(OH)2 at a pH of 10.00? (Ksp Mg(OH)2 is 1.6 x 10-13)
A: For a super saturated solution is taken and dissolved in water it gets ionised into its…
Q: What is the molar solubility of MgF2 in 0.36 M NaF? For MgF2, Ksp = 8.4 x 10–8. 7.1 x 10–4 1.0 x…
A:
Q: 1. Calculate the solubility (in M) of cobalt(II) hydroxide, Co(OH)2(s) in H2O. Ksp=2.60x10-16 at a…
A: All known compounds can be dissolve in certain solvents whereas they remain insoluble in other…
Q: What is the solubility of Mg(OH)₂ at a pH of 12.80? (Ksp Mg(OH)₂ is 1.6 × 10⁻¹³) __M
A:
Q: (Q57) What is the molar solubility of strontium fluoride in a solution that is also 0.0847 M in…
A:
Q: The value of Ksp for Cd(OH)2 is 2.5 * 10-14. What is the molar solubility of Cd(OH)2?
A: The solubility product of a particular compound is the product of the molarities of the ions present…
Q: The solubility of MgSO4 in H2O is 9.3 x 10^-3 mol/L. What's the KSP of MgSO4
A:
Q: The Ksp of Ba(IO3)2 at 25 °C is 6.0 * 10-10. What is the molar solubility of Ba(IO3)2?
A: Given Data:
Q: What is the solubility of Mg(OH)₂ at a pH of 11.60? (Ksp Mg(OH)₂ is 1.6 × 10⁻¹³)
A: Given pH = 11.60 As, pH + pOH = 14 So, pOH = 14 - pH pOH = 14 - 11.60 pOH = 2.40 Also, [OH-]…
Q: What is the solubility of Mg(OH)₂ at a pH of 10.20? (Ksp Mg(OH)₂ is 1.6 × 10⁻¹³)
A: Given data, pH of Mg(OH)2 = 10.20 Solubility constant, Ksp of Mg(OH)2 = 1.6 × 10-13
Q: What is the solubility of silver phosphate (418.58 g/mol) in pure water. Ksp = 2.6 × 10-18
A: Using the value of Ksp we can find the solubility of silver phosphate. Given Ksp = 2.6 × 10-18
Q: What is the molar solubility of Ag3PO4 ? Ksp = 2.64x10-18.
A: Ag3PO4 = > 3Ag+ + PO42-If x moles of Ag3PO4 dissolve 3x moles of Ag+ and x mole of PO4 is…
Q: What is the molar solubility of CaF2 (Ksp = 3.9 x 10-11)? A 6.24 x 10-6 M B 4.41 x 10-6 M 2.14 x…
A:
Q: The Ksp of calcium fluoride is 5.3 * 10^-9. What is the solubility of calcium fluoride in 2.72 *…
A: Solubility product is an ionic product at equilibrium
Q: What is the value of Ksp for MgCO3 (Molar mass: 84.3 g/mol) if its molar solubility is 2.4 x 10…
A: Given: Molar mass of MgCO3= 84.3g/mol Molar solubility= 2.4×10-3 To find: value of Ksp solution:…
Q: What is the molar solubility of Al(OH)3 in a solution containing 1.1 10-3 M NaOH? (ksp is 4.6 x…
A: NaOH dissociates as: [Na+] = [OH-] = 1.1× 10-3 M Al(OH)3 dissociates as: (Here solubility is…
Q: 11. What minimum mass of NaF must be added to a 1.0 L solution that contains 1.10 x 10 M Ba2* in…
A: Given data : 1.[Ba2+] = 1.10×10-2 M 2. Volume = 1L 3. Ksp = 2.4×10-5
Q: The Ksp for cobalt (II) hydroxide is 5.92x 10-15 at 25°C. What is the molarity solubility of Co(OH)2…
A: Given data,Ksp=5.92×10-15
Q: Please calculate the molar solubility of HgBr2 (K sp = 6.20 x 10-20 ) in a 2.58 molar FeBr3…
A: Given :: Ksp of HgBr2 = 6.20×10-20 [FeBr3] = 2.58 M molar solubility of HgBr2 = ?
Q: What is the solubility of MgCO₃ in a solution that contains 0.080 M Mg²⁺ ions? (Ksp of MgCO₃ is 3.5…
A: Use solubility product formula for AB type salt.
Q: The Ksp of Fe(OH)2 is 1.8× 10-15. What is the solubility of this salt in moles of Fe(OH)2 per liter…
A:
Q: What is the solubility (in M) of PbCl2 in a 0.15 M solution of HCl? The Ksp of PbCl2 is 1.6 x 10-5.
A: Solubility product is a type of equilibrium constant which value depends on the temperature. It is…
Q: What is the concentration of X- required (molarity) in a solution that is 0.0016 M in M+ in order to…
A:
Q: 6. The solubility of MgF2 in pure water is 0.0076 g/ per liter) of MgF, in 0,020 M NaF?
A: We have to find solubility product from the given data. We know that ksp value of compound is…
Q: what is the solubility in g/L of lead (II) iodide in water? the Ksp is 4.42 x 10 -9
A: Ksp = 4.42 × 10-9 Solubility of lead (II) iodide in g/L = ?
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- Give typed full explanation not a single word hand written otherwise leave it Calculate the pH during the titration of 40.00mL of 0.2000M propanoic acid (HPr, Ka = 1.3x10-5) after each of the following additions of 0.2000M NaOH (a) 0.00mL (b) 30.00mL (c) 40.00mL (d) 50.00mL0.2 mL of 0.10M NaOH is needed to titrate an unknown acid with a volume of 10.15mL. The final concentration of the resulting titrated sample is 0.163. Kindly explain how that value was found.13,How many milliliters of 0.0854 M NaOH are required to titrate 25.00 mL of 0.1250M HI to the equivalence point? Group of answer choices A, 17.08 B, 17.1 C, 36.6 D, no correct answer E, 36.593
- Exactly 50.00 mL of an HCl solution required 29.71 mL of 0.01963 M Ba(OH)2 to reach an end point with bromocreasol green indicator. What is the molarity of HCl?a student is preparing a Lactic acid (HLac) buffer (Ka= 1.4 X 10-4 , PH=4.00) answer the following questions: A. how many moles of conjugate base should be added to 315 mL of 0.45 M HLac to give a PH of 4.00? B. what is the ratio of the concentration of HLac to its conjugate base?5. One Erlenmeyer contains 50 mL of 0.1 M Na2CO3 solution, the other Erlenmeyer contains 50 mL of 0.1 M NaHCO3 solution. Answer the following questions when both solutions are titrated with 0.1 M HCl (F=1) solution separately: a) How much mL will be consumed if the phenolphthalein indicator is used? b) How much mL will be consumed if the methyl orange indicator is used?
- In an acid-base titration, 25.62 mL of an NaOH solution are needed to neutralize 26.23 mL of a 0.1036 M HCl solution. Use these steps to find the molarity of the NaOH. First note the value of MH+ in the HCl solution. Find MOH- in the NaOH solution. (MH+*Vacid= MOH-*Vbase ) Obtain MNaOH from MOH-How many millimeters of 0.0120 M NaOH are required to titrate 50.0mL of 0.0995M hydrofluoric acid to be the equivalent point? The K4 of hydrofluoric acid is 6.8 x 10-4 .How many grams sodium formate (HCOONa), 68.0069 g/mol) do you need to add to 250 mL of0.40 M formic acid (HCOONa) for a pH 3.5 buffer. Ka = 1.77 × 10 -4.
- Hello, I need help with the following question: You perform a titration using 25.0 mL of a 0.20 M propionic acid (HC3H5O2) as your analyte and 0.25 M NaOH as your titrant. Assume a new 25.0 mL of analyte is used for each step, determine the pH when the following volumes of titrantare used. (Propionic acid Ka = 1.32x10-5) a. 15.0 mL titrant added b. 25.0 mL titrant added Thank you.In a titration experiment, 14.50ml of 0.500M H2SO4 neutralize 40.0ml of NaOH. What is the concentration (molarity) is the NaOH solution?4.Suppose polyprotic acid H3X with Ka1=10-2, Ka2=10-5, Ka3 =10-10 . Answer the following questions for the buffer of 150 ml 0.1 M NaH2X and 50 ml 0.02 M Na2HX A) What is pH?B) Is the reverse reaction H2X-+ + H2O → H3X + OH- significant in determination of pH and why?C)Is the forward reaction HX2- + H2O → X3- + H3O+ significant in determination of pH and why?(Please do not use Henderson Hasselbalch equation!) Need answer for all three subparts Will definitely appreciate your efforts. Thank you.