Q: Which of the following is/are expected to be soluble in aqueous HCl? OH NH2 HN. Ph A D E Compound A…
A: HCl in water dissociate into H3O+ and Cl-. HCl + H2O = H3O+ + Cl-
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A: Given pH of solution is 5.56 ratio of [A-]/[HA] is .842 we have to determine Ka
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Q: what mass of solid lanthanum oxalate nonahydrate can be obtained from 650 ml of 0.0170 m aqueous…
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Q: Compare the molar solubility of Mg(OH)2 in pure water with that in a solution buffered at pH 9.00.
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Q: Iness is 250 mg/l as CaCO2 and alkalinity is 150 mg/1 as CaCO3.
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A: Balanced Chemical Equation: Sn3(PO4)2 (aq) + 6AgNO3 (aq) ———> 2Ag3PO4 (s) + 3Sn(NO3)2 (aq)…
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Q: Balanced chemical equation for conversion of Al(s) to KAl(SO4)2·12H2O(s) in aqueous solution
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Q: Compare the solubility of Zn(OH)2 in pure water with that in a solution buffered at pH 6.00.
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A: Given- 100 ml from water , pH = 8.1 '
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- Which is a weaker acceptor (analogous to weaker acid)? In, CuWhich is a weaker donor (analogous to weaker base)? As, MnIdentify the buffer capacity of the solution by titration using 0.250 M NaOH. Calculate the buffer capacity (β) of the phosphate buffer that have prepared using the data gathered below (see attached image): ΔpH = _____________________ ΔVNaOH = ___________________ Moles of titrant = ____________ Buffer Capacity (β) = _________C8This is for my reviewer please help me with the step by step solution and answer, thank you
- For water having a total alkalinity of 1.00x10^-3 mol/L and a pH of 10.34 what is the percentage contribution to alkalinity from CO32-? Please answer very soon will give rating surelyA buffer solution is formed by adding 0.200 moles of solid potassium nitrite, KNO₂, to 500.0 ml of 0.500 M Nitrous acid, HNO₂ solution. You may assume that the change in volume is negligible upon addition of the solid. pKa of HNO2 is 3.40 Ka of HNO2 is 4.0E-4 m.w. of HNO2 is 47.01 g/mol pH of the buffer solution is 3.30, so now Calculate the pH of the buffer solution after the addition of 5.00 ml of 2.50 M Ba(OH)₂.What species are present in a solution giving off a pure blue endpoint in a hard water sample containing an EBT indicator (In) with an EDTA titrant? a. HIn²⁻, CaY²⁻, MgY²⁻ b. HIn²⁻, MgIn⁻, CaY²⁻, MgY²⁻, CaIn⁻ c. HIn²⁻, MgIn⁻ d. HIn²⁻, MgIn⁻, CaY²⁻
- The pH of a 0.5L HNO2-NO2 buffer solution was determined to be 4.23. The solution was mixed with 5g of HNO2.Considering that the pKa is 4.35, what is the approximate pH of the new solution? Show all pertinent calculations.The MW of acid = 47g/mol. Illustrate the titration curve of the solution as a diprotic acid. Compute for the optimal pH if 1M of the solution isprepared. Illustrate what happens to the buffer system if additional acid or base is added to the solution. Label allparts accordingly.A 100-mL sample of hard water is titrated with the EDTA solution in Problem 2. The same amount of Mg2 is added as previously, and the volume of EDTA required is 31.84 mL. a. What volume of EDTA is used in titrating the Ca2 in the hard water? _____________mL b. How many moles of EDTA are there in that volume? _____________ moles c. How many moles of Ca2 are there in the 100 mL of water? _____________ moles d. If the Ca2 comes from CaCO3, how many moles of CaCO3 are there in one liter of the water? How many grams of CaCO3 are present per liter of the water? _____________ mol / L _____________ g / L e. If 1 ppm CaCO3 = 1 mg per liter, what is the water hardness in ppm CaCO3? _____________ ppm CaCO3I would really appreciate some help in confirming a value computed in a prelab problem to be used in a lab for analytical chemistry! We're working on redox reactions and are looking at the reaction: Fe2+ + K2Cr2O7 + H+ = Fe3+ + K+ + Cr3+ + H2O The final questions asks, "calculate the amount of unknown sample needed to achieve about a 25.00 mL titration volume of 0.01600 M K2Cr2O7 if the %Fe of the unknown is approximately 8%. Make sure to use the coefficients from the balanced reaction" I have found the balanced equation; however, I was hoping to be able to confirm my values! Thank you in advance!
- The conductivity of saturated solution of of BaSO4 is 3.48 x 10-4 S/m and the conductivity of pure water is 0.50 x 10-4 S/m at 298 K. Calculate the solubility product of BaSO4. ( limiting molar conductance of BaSO4 is 287.3 x 10 -4 S m2 mol.)The maximum buffering capacity is nearest to the pKa of the buffer. Explain why?The pKa of Cl3CCO2H is 0.64. What is the pH of a 0.580 M solution? What percentage of the Cl3CCO2H is dissociated? pH = ? = ? %