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A: Answer: Given that: pKb=9.5 As, -logKb=pKb-logKb=9.5logKb=-9.5on taking antilogKb=3.16×10-10…
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Q: Q what is the pH of abfor which has been prepard by mi sina 25 A,cl ae! 200 ,0 vnz sviukion ? what…
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Q: Calculate the pH for a 0.015 M (HC2H3O2) acetic acid solution. The Ka is 1.8 x 10 ^-5 for acetic…
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Q: The weak acid HZ has a Ka of 2.55x10-4.(a) Calculate the pH of 0.075 M HZ.(b) Calculate the pOH of…
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Q: A 0.419 M aqueous solution of monoprotic weak acid is measured to have a pH = 5.17. What is the…
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Q: 2-
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Q: What is the pH of a solution that is 0.33 M CH3NH2 (methylamine) and 0.52 M CH3NH3Cl (methylammonium…
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Q: Calculate the pH of a solution that contains 11% (w/w) NaOH and a density of 1.05 g/ml?, MW 40 O a.…
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Q: the pH and concentrations of species the following sõlutions (a) 0.20 M K,HPO4 An amphiprotic…
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Q: Determine the pH of a 0.588 M weak base soultions at 25C. The Kb for the weak base is 1.76 x 10^-5.…
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Q: Calculate the pH of 5.40 g of K2SO3 that has been completed with 500 mL H2O (pKa1= 1.85 and pKa2 =…
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Q: Calculate the pH at 25 °C of a 0.12M solution of sodium propionate (NaC,H,CO,). Note that propionic…
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Q: Calculate, at 25°C the [H+] and pH of tapwater sample in which the [OH-] = 2.0 x 10-7
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Q: The pKb of ammonia in water is 4.74. What is the pH of a 93.26 mL solution that contains 0.20 M…
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Q: For H2S, Ka1 = 9.6 10-8, and since Ka2 = 1.3 10-14, 0.04 M Na2S Calculate the pH of the solution by…
A: Given, Ka1 = 9.6×10-8 and Ka2 = 1.3×10-14
Q: For a temperature of 10C in which Kw= 2.89e-15 and Pkw = 14.539 what is the poH, ph H30+ ? OH=…
A: Applying concept of PHand POH. POH= - log [OH-]
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A: Given that: Activity of hydronium ion (aH3O+) = 0.0078549423 mol/L
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- Calculate the solubility of lead(II) sulfate (Ksp = 2.53x10-8) in a 0.0034 M solution of sodium sulfate. Give your answer to three sig. figs. and in exponential form (e. g. 1.23E-3).Calculate the solubility at 25°C of ZnOH2 in pure water and in a 0.0170M ZnSO4 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits.Calculate the solubility at 25°C of PbCO3 in pure water and in a 0.0110M PbNO32 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. solubility in pure water: gL solubility in 0.0110 M Pb(NO3)2solution: gL
- Calculate the solubility at 25°C of BaCrO4 in pure water and in a 0.0180M BaCl2 solution. You'll find Ksp data in the ALEKS Data tab. ksp for Ba Cr04 =1.17×10−10 Round both of your answers to 2 significant digits. solubility in pure water: gL solubility in 0.0180 M BaCl2 solution: gLCalculate the solubility at 25°C of Zn(OH)2 in pure water and in a 0.0080M ZnSO4 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. ksp of zn(OH)2 =3.0×10−17 solubility in pure water: gL solubility in 0.0080 M ZnSO4 solution: gLCalculate the solubility at 25°C of NiOH2 in pure water and in a 0.0020M NaOH solution. You'll find Ksp data in the ALEKS Data tab. ksp information is= Ni(OH)2 5.48×10−16 Round both of your answers to 2 significant digits. solubility in pure water: gL solubility in 0.0020 M NaOH solution: gL
- A 50.00 mL volume of 0.0600M K2CrO4 is mixed with 50.00 mL 0.0800 M AgNO3. Calculate the concentration of Ag+, CrO42-, K+, and NO3- at equilibrium. The solubility product of Ag2CrO4(s) is 1.20 x 10-12. Please show workBy the use of Henderson Hasselbalch equation; pH = pKa + log{[acetate ion]/[acetic acid]} 4.5 = 4.75 + log{[0.10 M]/[acetic acid]} -0.25 = log{[0.10 M]/[acetic acid]} [Acetic acid] = 0.10 M/ 10-0.25 [Acetic acid] = 0.10 M/0.56 [Acetic acid] = 0.1786 M Moles of sodium acetate dissolved in 250 mL buffer solution = 0.10 M× (250mL/1000mL) × 1L = 0.025 mol Weight (w) of sodium acetate (purity 100%) dissolved to prepare 250 mL of solution with buffer concentration of 0.10 M is calculate as follow; w100% = 0.025 mol × 82.0343 g/mol = 2.051 g Weight (w) of sodium acetate (purity 99%) is calculate as follow; w99% = 2.051 g× (100/99) = 2.072 g What was the volume of 6.12 M acetic acid HC2H3O2 needed to prepare the 250 mL acetic acid/acetate ion buffer solution required in this part? Show your calculations.Calculate the solubility of Ba(IO3)2 in pure water, Ksp=1.5x10^-9. Then calculate the solubility of the same Ba(IO3)2 in a 0.0025M Al(NO3)3 solution. Assume there is no other interatcion between any of the ionic componets of the 2 molecules. (do an activity coeffiecient problem using the neatest u value to determine f from the table)
- Suppose that CaF2 is to be used as a fluoridation agent in a municipal water system. What is the [F-] if extremely hard water ([Ca2+] = 0.070 M) is saturated with CaF2? (Ksp CaF2 = 1.7 x 10-10)(A) 1.3 x 10-5 M(B) 2.5 x 10-5 M(C) 5.0 x 10-5 M(D) 1.0 x 10-4 M(E) 0.070 M show work plsA sodium thiosulfate solution can be standardized by using it to titrate the iodine liberated by the action of excess KI on a known weight of primary standard K2Cr2O7: Cr2O72- + 6I- + 14H+ → 2 Cr3+ + 3I2 + 7H2O I2 + 2S2O32- → 2I- + S4O62- Calculate the molar concentration of the sodium thiosulfate solution if 31.47 mL of this solution were required to titrate a sample prepared using 0.2177 g pure K2Cr2O7.A 50 mL sample solution containing 8-hydroxyquinoline (MW: 145) was analyzed by adding 25 ml, 0.1 M KBrO3, excess KBr and acidified. The mixture was left for 10 minutes in dark place. After this time KI in excess was added followed by titration with 27.9 mL, 0.05 M thiosulfate standard solution. Write balance equations? What is the percent w/v 8-hydroxyquinoline in sample?