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- A 110.00 mL solution of 0.00195 M A3B2 is added to a 160.00 mL solution of 0.00155 M C3D4. What is pQsp for A3D2?Calculate the molar solubility of calcium oxalate in a solution that has been buffered so that its pH is constant and equal to 4.00. Data: Kps of CaC2O4 = 1.7x10 -9 ; Ka1 of H2C2O4 = 5.60x10-2 and Ka2 = 5.42x10-5 . Use systematic treatment.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⁻
- 0.3g of MBr is dissolved in distilled water to make 250mL in a standard flask. 25 mL ofthis is titrated with suitable indicator against 0.02 M silver nitrate solution and the end point was obtained at 12.8 mL of AgNO3 solution. Calculate the RMM of the metal bromide.The titration of 0.5001 g of KHP with a purity of 98.5% (204.223 g/mol) required 25.10 mL of NaOH. Calculate the concentration of NaOH solution KHP reacts with NaOH in a 1:1 ratio.Determine the molar solubility ( ? ) of Ag2CO3 in a buffered solution with a pH of 5.835 using the systematic treatment of equilibrium. ?sp(Ag2CO3)=8.46×10−12 ; ?a1(H2CO3)=4.45×10−7 ; ?a2(H2CO3)=4.69×10−11 .
- What is the molar solubility of Ag2CO3 in an aqueous solution that is buffered to a pH of 2.37? Relevant constants: Ksp for Ag2CO3 = 8.1 x 10-12; K1 H2CO3 = 4.45x10-7; K2 for HCO3- = 4.69x10-11; Kw = 1.00x10-14.If you would like to practice the Henderson-Hasselbalch calculations for the buffers in-lab exercise (attached) please use the following information for the buffer preparation: You are provided a 0.1M citric acid solution, a 0.1M sodium citrate solution and distilled water. You are to prepare a 50mL buffer at 25mM at a pH of 4.5. Citrate has three pKas at pH 3.128, 4.671, & 6.396.A solution contains 3.913g trichloroisocyanuric acid dissolved in 800mL citrate buffer with a pH of 12.5. How much 1M NaOH do you add to raise the solution's pH to 12.5? Please show detail, thank you.
- A 25.00 ml of Ni2+ solution was diluted in HCl and treated with 25.00 ml of 0.05283 MNa2EDTA. The solution was neutralized with NaOH followed by addition of acetate buffer untilthe pH 5.5. The solution turns yellow after addition of few drops of xylenol orange indicator.Back titration using standard 0.022 MZn2+ at pH 5.5 requires 17.61 ml until end point, onwhich the solution will turn red. Calculate for the molarity of the unknown.What is the molar solubility of PbBr2 in an aqueous solution containing (1.5x10^-1) M KBr? The Ksp of PbBr2 is 4.6 × 10-6 Note: Your answer is assumed to be reduced to the highest power possible.Tris or tris(hydroxymethyl)aminomethane is an organic buffering reagent most often used in nucleic acid extractions. Tris (MW = 121.14 g/mol) has a pKa of 8.07 at 25oC, with a white crystalline powder appearance. What is the buffering range/s of Tris buffer? How would you prepare 500mL of a 0.200 M Tris buffer solution using Tris and NaTris or sodium Tris (MW = 143.14 g/mol)?