Fe3+(aq)+ SCN–(aq) ⇄FeSCN2+(aq) Once the clear potassium thiocyanate was added, the mixture turned into a blood red color, but was still clear and all liquid, so in Le Chatelier's priniciple how was equlibrium affected when HCl was added
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Fe3+(aq)+ SCN–(aq) ⇄FeSCN2+(aq)
Once the clear potassium thiocyanate was added, the mixture turned into a blood red color, but was still clear and all liquid, so in Le Chatelier's priniciple how was equlibrium affected when HCl was added?
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- ○ 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.Fe3+(aq)+ SCN–(aq) ⇄FeSCN2+(aq) The color lightened so according to Le Chatelier's priniciple how was equlibrium affected when iron (III) chloride was added?Fe3+(aq)+ SCN–(aq) ⇄FeSCN2+(aq) The precipitate color was a cloudy white color with sime tint of orange so according to Le Chatelier's priniciple how was equlibrium affected when potassium thiocynate was added in additon to silver nitrate?
- 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!)1) Gallium hydroxide, Ga(OH)3, has a KSP of 7.28x10-36. Ga(OH)3(s) ⇌ Ga3+(aq) + 3OH-(aq)Under which circumstance will the [Ga3+] be the highest? Justify your answer.A) Dissolved into 1.00 L distilled waterB) Dissolved into 1.00 L of 1.00 M HClC) Dissolved into 1.00 L of 1.00 M NaOHWhat is the equilibrium constant of the following reaction at 25˚C?2AgBrO₃(s) + Li₂SO₄(aq) ⇄ Ag₂SO₄(aq) + 2LiBrO₃(aq)
- The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated:(a) TlCl: [Tl+] = 1.21 × 10–2 M, [Cl–] = 1.2 × 10–2 M(b) Ce(IO3)4: [Ce4+] = 1.8 × 10–4 M, [IO3−] = 2.6 × 10–13 M(c) Gd2(SO4)3: [Gd3+] = 0.132 M, [SO42−] = 0.198 M(d) Ag2SO4: [Ag+] = 2.40 × 10–2 M, [SO42−] = 2.05 × 10–2 M(e) BaSO4: [Ba2+] = 0.500 M, [SO42−] = 2.16 × 10–10 MSelect the shift in the reaction that is indicated by the change in color you observed. Then explain this change. Recall the reaction is as follows: Fe3+(aq)+NCS−(aq)⇌FeNCS2+(aq)pale yellowcolorlessred-orange color Observation: When Fe3+ was added, the Fe3+–NCS–FeNCS2+ equilibrium mixture turned darker red. A. Account for the effect of adding Fe3+, including a chemical reaction. B. Account for the effect of adding NCS-, including a chemical reaction. C. Account for the effect of adding Hg(NO3)2, including a chemical reaction. D. Molarity of FeNCS2+ in solution of “known concentration”Use the following information 2Fe(SCN)+2 (aq) ⇄ 2Fe(SCN)2+ (aq) + 2SCN- (aq) Kc = 0.1482 Fe(SCN)2+(aq) ⇄ Fe3+ (aq) + SCN- (aq) Kc = 1.124x10 -3 To determine the equilibrium constant (Kc) for the reaction Fe3+ (aq) + 2SCN- (aq) ⇄ Fe(SCN)+2 (aq)
- The following reactions all have K > 1.1) C9H7O4- (aq) + HF (aq) HC9H7O4 (aq) + F- (aq)2) CH3COO- (aq) + HF (aq) F- (aq) + CH3COOH (aq)3) HC9H7O4 (aq) + CH3COO- (aq) CH3COOH (aq) + C9H7O4- (aq)Arrange the substances based on their relative acid strength. CH3COOH HF F- C9H7O4- HC9H7O4 CH3COO- strongest acid intermediate acid weakest acid not a Bronsted-Lowry acid7) In the reversible reaction 2Cro? (aq) + 2H* (aq) E→Cr,0;² (aq) + H20 (I), chromium (VI) oxide (the reactant) is yellow and dichromate (the product) is orange. What will happen when you add concentrated HCI (aq) to the reaction mixture? a) The reaction mixture will become more yellow because increasing pH will shift the equilibrium to the left. b) The reaction mixture will become more yellow because decreasing pH will shift the equilibrium to the left. c) The reaction mixture will become more orange because increasing pH will shift the equilibrium to the right. d) The reaction mixture will become more orange because decreasing pH will shift the equilibrium to the right.Consider the following equilibria:Ca(OH)2(s) ⇌⇌ Ca2+(aq) + 2 OH-(aq) K1 = 6.5 x 10-6 H2O(l) ⇌⇌ H+(aq) + OH-(aq) K2 = 1.0 x 10-14Given these equilibria, what is the equilibrium constant, K, for the following reaction?Ca(OH)2(s) + 2 H+(aq) ⇌⇌ Ca2+(aq) + 2 H2O(l)