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- What is the molar solubility of AgI if its Ksp is 8.3 x 10-17? Please type answer note write by hend.A buffer is made up of equal volumes (451.8 mL of each) of 0.812 M A H and 0.885 M A minus. 24.51 mL of 0.712 M HCl is added to the buffer. How many moles of A H are present after the addition of HCl? Please use correct significant figures. Answer: (0.384) (mol)What volume of 0.50 M HNO3 should be added to 200ml of 0.20 M NH3 in order to creater a buffer with pH 9.00?. pKb(NH3)= 4.75. Express answer in two significant figures
- Situation: A 0.1214-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of 0.07011 M AgNO3, the sample was back titrated with 0.06021 M KSCN, requiring 27.15 mL to reach the end point. Questions: ONLY answer NUMBERS 3 and 4 Write the net ionic equations involved of the above titration process. Calculate the purity of the Na2CO3 sample based on the given above. The Ksp of AgCl is 1.82 x10-10 and the Ksp of AgSCN is 1.1 x10-12. Calculate the molar solubility of each express as mol Ag+/ L. What precipitate is more soluble? Is there a problem with this with reference to the titration above? And if there is, how will you remedy this?A buffer is made up of equal volumes (513.8 mL of each) of 0.846 M A H and 0.845 M A minus. 15.54 mL of 0.404 M N a O H is added to the buffer. How many moles of A H are present after the addition of N a O H? Please use correct significant figures. Answer: 0.428 MA laboratory manager wants to prepare 500.00 mL of a buffer with a pH of 4.471 from equimolar solutions of CH3CO2H (Ka = 1.800e-5) and LiCH3CO2. What volume of the LiCH3CO2 solution would be required? Key Concept: Buffers resist pH change and are prepared by mixing the conjugate acid and base together. The pH is determined from the Henderson-Hasselbach equation: pH = pKa + log([A−]/[HA]).Solution: Since the molarities of the two solutions making the buffer are the same, the Henderson-Hasselbach equation can be written as: pH = pKa + log(V(A−)/V(HA)) where V(A−) = the volume of the conjugate base and V(HA) = the volume of the conjugate acid.
- Solid cobalt (II) acetate is slowly added to 125 mL of 0.0945 M ammonium chromate solution. What is the concentration of cobalt required to just initiate precipitation? The Ksp of CoCrO4 is 7.1 * 10 -4. Report answer in scientific notation to two sig figs.In the standardization of NaOH with potassium hydrogen phthalate (KHP). A known amount of KHP is weighed and dissolved in water. This is then titrated incrementally with NaOH from a buret until the phenolphthalein changes color from colorless to pink. Which is the titrand? a.cannot be determined form above scenario b.HCl c.NaOH d.phenolphthalein e.KHPIn lab, you will be provided with a 1.8 M acetic acid solution (CH3COOH) and solid sodium acetate trihydrate (NaOOCCH3 3H2O). You want to make 100.0 mL of a 0.5 M acetic acid buffer at pH 5.00. How many grams of sodium acetate trihydrate, and what volume (mL) of the 1.8M acetic acid solution and deionized water should you combine? The pKa of acetic acid is 4.75. Show all work.
- Calculate the molar solubility of lead bromide, PbBr2 (Ksp = 4.0×10–5)molar solubility = Answer mol/LCalculate the pH of a saturated solution of manganese (II) hydroxide, Mn(OH)2, (Ksp = 1.9×10–13)pH = AnswerA buffer is made up of equal volumes (468.3 mL of each) of 0.860 M A H and 0.884 M A minus. 29.32 mL of 0.399 M N a O H is added to the buffer. How many moles of A minus are present after the addition of N a O H? Please use correct significant figures. Answer: (0.426) (mol)Situation: A 0.1214-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of 0.07011 M AgNO3, the sample was back titrated with 0.06021 M KSCN, requiring 27.15 mL to reach the end point. What is the net ionic equations involved of the above titration process?