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- When comparing a solution of HNO3([HNO3=0.3M]) and a solution of H2SO4 ([H2SO4 = 0.3M]) - which solution would have most acidic pH3. What is observed when the H2O concentration in the acetic acid equilibrium becomes relatively low? Relatively high? 4. Humidity indicator cards (HIC) are commonly added to semiconductor shipments to document that the parts were not exposed to humidity. These cards are impregnated with cobalt(II) chloride, or an alternative, and change color to indicate the presence of water. Predict the color you would see if a cobalt(II) chloride HIC were exposed to moist, humid air?When the reaction below reaches equilibrium, does the equilibrium lie on the left or the right side? Briefly explain.ClO– + CH3CO2H ⇌ HClO + CH3CO2–
- For the following reaction, the products are favored at equilibrium. Classify each of the reactants and products based on their strength as Bronsted-Lowry acids or bases.C5H11N + C6H5COOHC5H11NH+ + C6H5COO- C6H5COO- C5H11N C5H11NH+ C6H5COOH Stronger Bronsted-Lowry acid Weaker Bronsted-Lowry acid Stronger Bronsted-Lowry base Weaker Bronsted-Lowry baseWrite a chemical equation for the hydrolysis reaction that explains why an aqueous solution of CH3NH3Cl is acidic. [Please include the states of matter with each chemical species. Remember, it is an equilibrium reaction.]- Calculate the pH of a 0.102 M solution of ethylenediamine (H, NCH₂CH₂NH₂). The pK, values for the acidic form of ethylenediamine (H; NCH₂CH₂NH) are 6.848 (pK₂1) and 9.928 (pK2). pH = Calculate the concentration of each form of ethylenediamine in this solution at equilibrium. [H₂NCH₂CH₂NH₂] = [H₂NCH₂CH₂NH] = [H; NCH₂CH₂NH] = M M M
- Use the following reaction and information to answer a and b. 2ClO2(aq)+2OH-(aq)-->ClO-(aq)+Cl2-(aq)+H2O(l) [ClO2](M) [OH-](M) Initial rate (M/s) 0.060 0.030 0.0248 0.020 0.030 0.00276 0.020 0.090 0.00828 a. What is the order of this reaction in respect to ClO2, with respect to OH-, and the overall order? Assume the rate law has the form rate=k[ClO2]a[OH-]b b. What is the value of the rate constant? Include the units and why the unit make sense.Which of the statements below best describes this equilibrium: HCIO4 + CH3CO2 CIO4 + CH3CO₂H Note: the Ka of CH3CO₂H is 1.8 x 10-5 This is a product-favored equilibrium and the final solution is acidic This is a product-favored equilibrium and the final solution is basic This is a reactant-favored equilibrium and the final solution is acidic O This is a reactant-favored equilibrium and the final solution is basicSelect the outcome of the following reaction. Br2 Br Br only Br only Brm Br Br