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- . Use stoichiometry to determine the equilibrium [Fe3+] and [SCN-] in each test tube. y = 6170.7x - 0.0153 Solution 0.002M iron(III) nitrate in 1M nitric acid(mL) 0.002M potassium thiocyanate(mL) DI water(mL) Absorbance(A) 1 3 2 1 0.128 2 2 3 1 0.2694.) Consider the following equilibrium: Fe3+(aq) + SCN"(aq) = FESCN2+(aq) Initial concentrations: [Fe3+] = 0.390; [SCN"] = 0.819; [FeSCN2+] = 0 The equilibrium concentration of [FESCN2+]eg = 0.300 M. What is the equilibrium concentration of Fe3+? [Fe3+]eq =5.) Consider the following equilibrium: Fe3+(aq) + SCN"(aq) = FESCN2+(aq) Initial concentrations: [Fe3+] = 0.150; [SCN] = 0.315; [FESCN2+] = 0 The equilibrium concentration of [FESCN2+]eg = 0.115 M. What is the numerical value of Kc for this equilibrium?
- imagine that you have passed general chemistry with flying colors and are now doing undergraduate research for me. Once you stop dancing for joy (because you got an A, of course), considerer the following reaction: NiCl2 + 6NH3 + 2 KClO4 --> Ni(NH3)6(ClO4)2 + 2KCl if you mix 1.0406g of NiCl2, .0092g NH3 and 2.0008g of KClO4 how many g of KCl form?When barium fluoride dissolves in water at 25 °C, the equilibrium concentration of Ba2+ is 3.6*10-3 M. Use this information to calculate Ksp for BaF2.Write the Ksp expression for the sparingly soluble compound barium phosphate, Baz(PO4)2. Ksp = A₂ If either the numerator or denominator is 1, please enter 1
- (a) In the determination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in mg/L., on the basis of the solubility product principle, when the chloride concentration has been reduced to 0.2 mg/L? (b) If the concentration of chromate indicator used is 5 x 10-3 M, how much excess silver ion in mg/L. must be present before the formation of a red precipitate will begin?Consider a receptor (R) that binds two ligands (L & M ) in a sequential fashion. For example, ligand "L" must be present before ligand "M" can bind. In dissociation reactions, it would look like this. R•L•M R•L + M with equilibrium constant Kam R•L OR+L with equilibrium constant Ka a. Derive an equation that relates the fraction [R•L•M]/[R]tot to the concentrations of free L and free M. b. In terms of the dissociation constant, Kam, what concentration of ligand "M" will lead to 50% of the receptor existing in the R•L•M state when [L] = 10 x Ka?○ Ni(H₂O)²+(aq) + 3SCN- (aq) = Ni(SCN)3(aq) + 6H₂0(1) (a) Write the Kc expression for this equilibrium. (b) Would there be a shift to the right or to the left if KSCN solution was added to a solution containing this equilibrium? Explain your answer.
- Use the systematic treatment of equilibrium to calculate the concentration of Ba2+ in acidic solution, if its concentration is governed by the following equilibria – BaSO4 (s) → Ba2+ + So Ksp = 1.1 x 10-10 so, +H2O HSO, +OH K, = 9.8 x 10-13 Bat + So, BaSO4 (aq) K = 1.9 x 10 Hint: Since the pH is fixed at 1.89, the charge balance is invalidated. Use the mass balance for your calculation.3) One of the main buffer systems found in living organisms is the phosphate buffer system, often used in biological research to mimic cellular conditions. The phosphate equilibrium reactions and their corresponding pKa's are as follows: H3PO4 = H* + H2PO, H2PO, = H+ + HPO?- HPO- = H+ + PO;- pKa1 pКаz —D 7.21 = 12.44 = 2.12 pKa3 (a) Given the above chemical reaction, write out the expression for K, of the buffer system which would predominate at neutral pH conditions. Justify your choice. (b) The human body, and many other lifeforms, prefer an internal pH of 7.2 to maintain homeostasis. However, some more acid-tolerant or basic-tolerant organisms can survive (and sometimes thrive) within different ranges of pH. Calculate the mass and moles of the correct acid and corresponding conjugate base solid (assume you have sodium salts of each base: NaH,PO4, Na,HPO4, and Na PO,) which are needed to make 500 mL of a 0.5 M buffer solution (0.5 M total, including the concentration of acid and base…Construct the expression for Kc for the following reaction. FeO(s) + H,(g) = Fe(s) + H,O(g) 1 Drag the tiles into the numerator or denominator to form the expression. Ke SRESET [FeO] 2[FeO] [FeO]? [H] 2[H] [HJP [Fe] 2[Fe] [Fe]? [H.O] 2[H,O] [H,O? II