At this point, [Cl-] is governed by the Ksp reaction. We can make this a really easy calculation by simply assuming that we are starting from no dissolved Ag+ and Ci", but instead only solid AgCl. We can then calculate what the Ag* and Cl- concentrations are at 10 mL Ksp = 1.8 x 10-10 = [Ag*l[Cl¯] You have solved this kind of problem many times now. Do it again for [Cl"] for the 10 mL.
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- Please watch this video and solve the following two questions ( https://www.youtube.com/watch?v=ojZ9hpi-9w0&t=29s ) "preparation of aspirin" -What is the purpose of the concentrated sulfuric acid used in the first step? -Hydrochloric acid is about as strong a mineral acid as sulfuric acid. Why would HCl not be a satisfactory catalyst in this reaction?virtual experiment setting the pH Buffer to 4.4 and the temperature to 45 oC keeping all other concentrations at the default setting. a) Suggest a reason why the "stopwatch" method of measuring the reaction rate would be unsuitable under these conditions. b) When conducting experiments on the temperature dependence of a reaction, why is it important to use the same concentrations for each different temperature?A saturated AgClAgCl solution was analyzed and found to contain 1.25 x 10-5 M Ag+AgX+ ions. Use this value to calculate the Ksp of AgCl
- What is the ratio of the moles of sodium hydroxide to the moles of crystal violet (nNaOH/nCV+) at the start of the reaction? Make sure to account for the fact that different volumes of the stock solutions are mixed. 5.0 mL 2.0 × 10–5 M crystal violet solution 1.0 mL of 0.10 M NaOH solution Trail. [Na+]j (M) [OH–]j (M) 1 1.67 × 10–2 1.67 × 10–2Magnesium fluoride (MgF2, MW = 62.30 g/mol) is slightly soluble in water, with Ksp = 7.4 x 10^-11 at T= 25. C.a) Give the correctly balanced solubility reaction and expression for Ksp for MgF2.b) What mass of magnesium fluoride will dissolve in 1.000 L of pure water?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).
- 8.00mL aqueous suspension of elemental selenium is treated with 24.00mL ammonia 0.045M AgNO3 The reaction is as follows: 6Ag (NH3) 2 ++ 3Se (s) + 3H2O → 2Ag2Se (s) + Ag2SeO3 (s) + 6NH4 + After this reaction is completed, nitric acid is added to dissolve Ag2SeO3. However, Ag2Se does not dissolve during this time. Ag + consisting of dissolved Ag2SeO3 and the excess of the reagent requires 13.43mL 0.01294M KSCN in a Volhard titration. How many milligrams of Se are in each milliliter of sample? (Se = 78.96g / mol)The Ksp of Pb(OH)2 at 25 °C is 1.4 x 10-15. What concentration of NaOH will commence precipitation of Pb(OH)2(s) from a solution that contains 0.025 mol L-1 Pb2+(aq) ion?Potassium dichromate has several industrial applications. To determine the purity of the salt that will be used in different industrial processes, a sample mass equal to 2.660 g was dissolved and quantitatively transferred to a 500.00 mL flask. An aliquot of 25.00 mL of this solution was treated with excess KI and the released iodine was titrated with 0.1000 mol L-1 sodium thiosulfate, spending 27.00 mL. Calculate the purity of the analyzed salt. Data:K = 39.10 O = 16.00 Cr = 52.00 I = 126.9 S = 32.07
- How would the equilibrium be affected in regards to the value of Qc or Kc for each of the following conditions?: Fe3+ (aq) + SCN- (aq) ⇌ FeSCN2+ (aq) Adding KSCN (aq) Adding Fe(NO3) (aq) Adding NaF (s) Placing the solution into a hot water bath Placing the solution into an ice bath (To whom this may concern, Could you at least explain one as simply as possible so I'm able to understand the others enough to explain them myself? Thanks in anvance!)What amount of NH4Cl must be added to prevent precipitation of Mg(OH)2 from a 1L solution that is 0.050M in Mg2+ and 0.050M in NH3.? Ksp of Mg(OH)2=2.06x10-13.This reaction must have a ∆G<0 at SATP: Xe(g)+F2(g)→XeF2(g) 2Na(s)+Cl2(g)→2NaCl(s) 2NaF(s)+I2(s)→2NaI(s)+F2(g) MgSO4(s)→Mg(s)+S(s)+2O2(g)