Calculate all the concentrations in equilibrium in a 0.4M solution of magnesium hydroxide magnesium hydroxide = [Select] magnesium ion = [Select] hydroxide ion [Select] = hydronium ion = [Select] > < У М M M У М
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![Calculate all the concentrations in equilibrium in a 0.4M solution of
magnesium hydroxide
magnesium hydroxide = [Select]
magnesium ion = [Select]
hydroxide ion [Select]
=
hydronium ion = [Select]
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- The equilibrium of hydroniumn ion concentrations of an initially 0.253M solution of a monoprotic weak acid is 2.2x10^-3M. The acid dissociation constant is 1.91 x 10^-5 at 25C. What is the pH of the solution?A solution of sodium acetate is prepared using 0.56 mol L-1 NaOH as the solvent. The pKapKa of acetic acid is 4.75 . The concentration of sodium acetate after mixing, before any reaction takes place is 0.44 mol L-1 . Calculate the equilibrium concentrations of all acid species: [ CH3COOH ], [ CH3COO- ], the pH and the pOH in the solution. Some assumptions may not work, on the other hand, if you do not make the correct assumptions first, the quadratic formula will give you the wrong answer. [ CH3COOH ] = ___mol L-1 , [ CH3COO- ] = ___mol L-1 , pH = ___ pOH = ____54.9mL of 0.132 M hydrochloric acid is added to 133.7mL of 0.069 M pristine solution What is the appropriate pH?
- What is the concentration of H3O+ in a solution that is 0.0600 M Hypochlorous acid (HClO)? What is the pH? To solve this problem: Write the acid dissociation equilibrium for HClO Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, ClO- and HClO at equilibrium, in terms of x. Decide if x can be neglected. You may neglect x if the initial concentration of the HClO is greater than 100 times the Ka. You will need the value of Ka. Look it up on the chart (p 4 of packet) Solve for x Find the pH The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic aicd “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it…Consider a mixture of 1.36 M HCIO and 1.65 M NaCIO. Given that the K, for HCIO = 2.9 x 10-8 determine the pH of this solution.Considering the equilibrium below, which of the following is/are TRUE? CH3OH + HNO2 = CH3OH2+ + NO2- CH3OH is a base NO2 is a conjugate acid IAM. I only SXY. II only AND. I and II IKI. Neither I nor II Which of the following statements is/are ALWAYS TRUE? A higher Ksp value equates to a higher solubility regardless of the salt type When Qsp = Ksp, the system is at equilibrium CHM. I only EQU. II only LIB. I and II RIA. Neither I nor II
- An aqueous solution contains 0.397 M ammonia. Calculate the pH of the solution after the addition of 4.63 x 10-2 moles of perchloric acid to 250 mL of this solution. (Assume the volume does not change upon adding perchloric acid). Ka = 5.6 x 10-10, Kb = 1.80 x 10-5Calculate the pH of a solution that is 0.080 M pyridine (pKb = 5.25) and 0.285 M pyridinium chloride.A 0.025 M solution of an unknown organic acid has a pH of 3.23. 2.1 By means of a full calculation, determine the value of the ionisation constant of the conjugatebase of this acid..- You may use “HA” to denote the formula of the acid.- You may make certain assumptions to simplify your calculations2.2 A certain amount of the sodium salt of the conjugate base of the acid was added to the system.Will the pH of the resulting solution increase or decrease, compared to the original given value? Explain your answer in a short sentence or two.
- Calculate the pH of a mixture containing 0.23 M HONH2 and 0.44 M HONH3Cl. (Kb = 1.1 × 10–8) What information do we need to calculate the pH? (Choose all letters that apply.) a. 0.23 M HONH2b. 0.44 M HONH3Clc. the major species in the solutiond. pOH = –log[OH–] and 14.00 = pOH + pHe. Kb = 1.1 × 10–8Derive and equation analogous to the Henderson-Hasselbalch equation but relating poH and pKb of a buffered solution composed of a weak base and it conjugate acid, such as NH3 and NH+4Without neglecting the pH of the solution containing 0.04 M H3PO4Find. Ka1 = 7x10-3Ka1 = 2.2x10-7Ka3 = 4.5x10-13) Note: The corresponding balancewrite the reaction, state the equilibrium constant.