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- Cr2O7 2- (aq) + 14H+ 6e- ---> Cr3+(aq) + 7H2O(l) Ered = 1.33V Cu2+(aq) + 2e- --> Cu(s) ?°red = 0.34V Determine the Ecell at 25°C, given: [Cr2O7(aq) 2- ] = 0.2500M ,[Cr(aq) 3+ ] = 0.2500M , pH =5 [Cu2+]=0.2500Mplz asap give typed answer with step by step explanationWhat is Kb for the equilibrium rreacton: CN- + H2O <=> HCN + OH- ? Ka value of 6.23 x10-10
- determine the Kb for CN- at 25°C. the Ka for HCN is 4.9 x 10^-10direct to the point answers plsHoping for solutions since I’m having a hard time with this. Pls skip if unsure or not willing to answer the subitems (these are all connected for one item). Thanks in advanced. Kriel just discovered a new protein, Krielase and for it not to unfold and lose its function, he realized that the protein needs to be constantly immersed in a pH = 6.50 solution. He is therefore interested in preparing a 50 mL 0.08 M pH = 4.50 buffer to contain the protein. He listed down the pure acids available to his disposal, and also looked for their acid dissociation constant (Ka) values. Acid Name Ka1 Ka2 Ka3 Nitrous Acid (HNO2) 4.00 x 10-4 N/A N/A Acetic Acid (CH3COOH) 1.76 x 10-5 N/A N/A Ascorbic Acid (HAsc) 7.90 x 10-5 1.60 x 10-12 N/A Phosphoric Acid (H3PO4) 7.52 x 10-3 6.23 x 10-8 4.28 x 10-13 A. Identify which weak acid system is best to use in preparing the buffer? Why? B. Identify the species which will make up the buffer system?…
- (9.29 × 105/8)-20.81 = with correct sig figsIf an Ecell of 0.495V was noted when your cell was set-up. What is thesolution pH?Which of the following is a spontaneous reaction.? a. Rxn with ΔH =- 10Kj/mol ΔS= -5J/mol T= 300K b. NaCl +H20 -> NaOH + HCl 25C c. H20(l) -> H2O(s) Temp: 25C d. Dissolution of 100g of solid sugar in 100 mL ice tea. Consider following reaction: HgO (s) -> Hg(l) + ½ O2 (g) Delta H = +90.7 kj/mol. What quantity of heat in kj/mol is required to produce one mole HgO? Write your answer without units. Given the following data 2ClF(g) + O2(g) --> Cl2O(g) + F2O (g) Delta H= 167.4 kJ I 2ClF3(g) + 2O2(g) --> Cl2O(g) + 3F2 O (g) Delta H= 341.4 kJ II 2 F2(g) + O2(g) ---> 2F2O (g) Delta H= -43.4 kJ III Calculate the delta H in kJ for below reaction: ClF(g) + F2(g) ---> ClF3(g)
- please help me solve tghe following question and explain pls, its important, thanks!!Acetic acid (CH3COOH, abbrev. HA) is a very common weak acid with pKA = 4.75 (at 25oC and low ionic strength). Calculate pH of the diluted solution of acetic acid with concentration c = 0.05 mol dm-3.Hexanoic acid was added to an immiscible biphasic solvent sysem, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D1) of hexanoic acid in CCl4 with respect to water.