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- Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?What is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.. The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of Fe(OH)3in moles per liter and in grams per liter.
- The ore cinnabar (HgS) is an important source of mercury. Cinnabar is a red solid whose solubility in water is 5.5 X 10-2 mol L-1. Calculate its \p. What is its solubility' in grams per 100 g of water?Why are there no changes specified for NH4HS in Exercise 13.62, part (e)? What property of NH4HS does change?Peptide decomposition is one of the key processes of digestion, where a peptide bond is broken into an acid group and an amine group. We can describe this reaction as follows: Peptide(aq) + H2O(l) ⇆acid group(aq) + amine group(aq) If we place 1.6 mol peptide into 1.0 L water, what will be the equilibrium concentrations of all species in this reaction? Assume the K value for this reaction is 3.1 × 10-5. [peptide] = M? [acid group] = M? [amine group] = M?
- Subject: chemistry Watch this video about chemical equilibrium and explain to me step by step on whats happening in the video with long explanation must be long and detailed and easy to understand/ an explanation of whats happening and its conclusion https://youtu.be/YMsiLbKXbp4Reaction: CrO42-(aq)+2H+(aq) <--> Cr2O72-(aq)+H2O(l) YELLOW ORANGE If sulfuric acid (H2SO4) is added to this solution, will a color change be observed? If so, how does the addition of sulfuric acid result in a color change? Explain your reasoning by showing the effect of the addition of H2SO4 on the equilibrium for the reaction.Consider the insoluble compound zinc carbonate , ZnCO3 . The zinc ion also forms a complex with hydroxide ions . Write a balanced net ionic equation to show why the solubility of ZnCO3 (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction.For Zn(OH)42- , Kf = 2.9×1015 . Be sure to specify states such as (aq) or (s). + + K =
- The equilibrium at 25 °C MaCl5 (aq) + 4 H2O (l) ↔ H3MaO4 (aq) + 5 HCl (aq) Kc = 5500 ΔH°(rxn) = 28.1 kJ/mol, Determine the ΔG°(rxn)The KspKsp of a salt corresponds to a reaction with the following general format: salt(s)⇌mcation(aq)+nanion(aq)where mm and nn are the coefficients that balance the equation. Equilibrium constants follow the general format of products over reactants (excluding pure liquids and solids) with each species raised to the power of its coefficient in the balanced equation. KspKsp is no exception, so Ksp=[cation]m[anion]nKsp=[cation]m[anion]n Part A If 500.0 mLmL of 0.10 mol L−1 Ca2+mol L−1 Ca2+ is mixed with 500.0 mLmL of 0.10 mol L−1 SO42−mol L−1 SO42−, what mass of calcium sulfate will precipitate? KspKsp for CaSO4CaSO4 is 2.40× 10−52.40×10−5. Express your answer to three significant figures and include the appropriate unitsWe have a hot tub that uses ozone (O3) gas as a disinfectant. The ozone generatorbubbles ozone in the water and it has a concentration of 2 mg/L of dissolved ozone in the water. I’mconcerned that the headspace above the water will have a high concentration of ozone which can behazardous. For example, OSHA states that the maximum permissible exposure is 0.2 ppmv for a 2hour exposure. Will the equilibrium ozone concentration in the headspace above the water exceedthis limit? The Henry’s Law constant for ozone is:O3(g) ↔ O3(aq) KH = 9.4 x 10-3 mol/L-atm