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Q: of
A: Dear student I have given answer to your question in the image format.
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please answer 2nd quesion
when a nonvolatile solute dissolves in water to form a solution?
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- A dilute solution of NaOH is titrated with 0.9050 g primary standard potassium hydrogen phthalate (KHP, C8H5K04, FW=204.23 g/mol) which required 10.50 mL of the base using phenolphthalein indicator. (a) What is the color at the endpoint? (b) What is the molar concentration of the titrant?A 25 mL solution of 0.255 M AgNO3 titrant was added to a 50 mL sample that contains chromate ion (CrO4 2-). It required 12.39 mL of a 0.1998 M thiocyanate (SCN- ) solution to titrate to a red point. What is the concentration of the chromate ion in ppm and molarity?5 SO2 + 2 MnO4- + H2O ---> 5 SO42- + 2 Mn2+ + 4 H+ The MnO4- solution is poured in a burette and then titrated till the equivalent point is aquired. How many L are needed of MnO4? (the burette starts at 5,7 and is 37,3 after titration)
- The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. A. What is the pH at the beginning of the titration, Vbase = 0.00 mL? B. What is the pH at the equivalence point? C. What is the pH of the titration when 5.00 mL of base have been added? D. What is the pH when the volume of base added equals half the volume of the equivalence point? E. What is the pH of the titration when 20.00 mL of base have been added? F. What is the pH of the titration when 30.00 mL of base have been added?Consider the titrimetric determination of acetic acid (60.05 g/mol) in vinegar. Titration of a 5.00 mL vinegar sample requires 12.15 mL of 0.250 M NaOH to reach the phenolphthalein endpoint. How many grams of acetic acid are present in the sample? 0.930 1.08 0.242 0.182 None of the choicesThe Ksp of PbBr2 is 6.60×10-6 M3. - What is the molar solubility of PbBr2 in pure water? - What is the molar solubility of PbBr2 in 0.500 M KBr solution? - What is the molar solubility of PbBr2 in a 0.500 M Pb(NO3)2 solution?
- Consider the titrimetric determination of acetic acid (60.05 g/mol) in vinegar. Titration of a 5.00 mL vinegar sample requires 14.25 mL of 0.150 M NaOH to reach the phenolphthalein endpoint. What is the molarity of acetic acid? choices 1.24 0.808 0.428 0.0526Neutralization Titration In the standardization of HCI solution using 10.00 ml of 0.02 Na,co, according to the equation M of Na,CO, 2 HCI 2NaCl + H₂O+CO, 15.0 ml of HCI is required to reach the end point using Bromocresol green indicator the molarity of HCI (mol/L) would be al 0.032 b) 0.027 20.013 d) 0.008 e) 0.064The answers to the questions are already given. Please show the solution how to get the answers. A solution containing 0.5 mM CO32- and 2.5 mM F- is to be separated using Mg(NO3)2 as precipitating agent. Ksp of MgCO3=3.5x10-8. Ksp of MgF2=3.7x10-8. Which ion will precipitate first? Answer: CO32- How much of the first ion (in M) will be left when the second ion starts to precipitate? 5.91x10-6 M
- What is the cobalt(II) ion concentration in a solution prepared by mixing 357 mL357 mL of 0.396 M0.396 M cobalt(II) nitrate with 475 mL475 mL of 0.399 M0.399 M sodium hydroxide? The ?spKsp of cobalt(II) hydroxide is 5.92×10−155.92×10−15 .In the lab you mix 75 mL of NaOH solution with a pOH of 2.45, with 125mL of a 0.018 M solution of MgCl2. The Ksp of Mg(OH)2 is 2.06*10^-13. A. Write the total ionic equation for the system. B. What is the Qsp? C. Do you expect a precipitate to form?The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. a) Sketch the pH vs volume of added base titration curve for this reaction. pH vertically, volume of base horizontally. Label your axes with correct pH and volumes. (Attach more space, if needed) b) what is the pH at the beginning of the titration, Vbase = 0.00 mL ? c) what is the volume of the base needed to reach the equivalence point ? (label the equiv. point) d) what is the pH at the equivalence point?e) what is the pH of the titration when 5.00 mL of base have been added ? f) what is the pH when the volume of base added equals half the volume of the equivalence point? g) what is the pH of the titration when 20.00 mL of base have been added? h) what is the pH of the titration…