Consider the following equilibrium reaction:H₂O + H₂O2 H₂O+ + OH¯When Sr(OH)2 is added, the equilibrium will shift to theA. left and H₂O* decreases.left and [H3O+] increases.B.C. Nothing shifts. No Change in EquilibriumD.right and [H3O+] increases.E.right and [H3O+] decreases.

Given , Reaction : H2O + H2O ⇌ H3O+ +OH-When , Sr(OH)2 is added, the Sr(OH)2 dissociates in aqueous solution as : Sr(OH)2→Sr2++2OH- As , Sr(OH)2 gives OH- in the solution , and in the given reaction OH- is on product side , so addition of Sr(OH)2 increases OH- concentration in the given aqueous solution , hence according to Le-chattelier principle (introducing any disturbance to the system at equilibrium will tend to shift the equilibrium to the direction which undoes the effect caused by the disturbance ), the equilibrium will shift towards reactants side or the left side , as now as equilibrium is constant value , so if we increase the concentration of OH- , the concentration of H3O+ will decrease. Hence adding Sr(OH)2 to the reaction equilibrium will shift the reaction to left side and H3O+concentration will decrease. So, correct option is (A)

Science

Chemistry

Consider the following equilibrium reaction: H₂O + H₂O H₂O* + OH¯ When Sr(OH)2 is added, the equilibrium will shift to the OA. left and H30* decreases. left and [H3O+] increases. O B. O C. Nothing shifts. No Change in Equilibrium O Dright and H3O* increases.

Consider the following equilibrium reaction: H₂O + H₂O H₂O* + OH¯ When Sr(OH)2 is added, the equilibrium will shift to the OA. left and H30* decreases. left and [H3O+] increases. O B. O C. Nothing shifts. No Change in Equilibrium O Dright and H3O* increases.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Hydrogen iodide dissociates according to the equation 2HI(g) <=> H2(g) + I2 (g). A 0.2 moles of gaseous hydrogen iodide was placed in a 200 ml flask. At equilibrium it was found that 20% of the HI had dissociated. What is the Keq or Kc value for the equilibrium system? a. 1/4 b. 1/8 c. 1/16 d. 1/64
0.60 moles of H₂ and 1.4 moles of S are placed into a 2.0L flask and allowed to reach equilibrium. Calculate the [H₂] at equilibrium. _H2 (g) + _S (s) _H₂S (g) Keq= 14
I need help woth both pless
Hi, Write an equilibrium expression for the chemical equation involving one or more solid or liquid reactants or products. CO32- (aq) + H2O(l) <-----> HCO3(aq) + OH-(aq) Thanks,
When a reaction is said to have reached equilibrium, it means A- The reaction in both directions have stopped. B- The rate of the forward reaction is higher than that of the reverse reaction. C- The concentration of reactant and product are equal. D- The concentration of reactant and products do not change over time. E- The rate of the forward reaction is lower than that of the reverse reaction.
Consider the following reaction at equilibrium: 2CO2 (g) 2CO (g) + O2 (g) H = -514 kJ Le Chatelier’s principle predicts that __________will result in an increase in the number of moles of O2
title=q10a8 What conclusion can you make about the position of equilibrium for the following reaction? A BAG = +1.0 kJ/mol the ratio of B to A will be less than one O the ratio of B to A will be greater than one O the ratio of B toA will be exactly 1 O the ratio of B to A will be exactly -1 O no conclusions can be made about the ratio of B to A from the information given
What effect does each of the following changes have on the equilibrium of the reaction: (left or right) 2SO2 (g) + O2 (g) → 2 SO3 (g) + heat a. remove O2 b. raise temperature C. add SO2 d. remove SO3
1. Note: Please don't write on a paper. I can't understand handwritten.
If the reaction quotient (Q) is greater than the equilibrium constant (K) for a reaction then O a. the reaction can proceed both forward and backward directions. O b. the reaction will stop. O c. the reaction will proceed toward reactants. O d. the reaction will proceed toward products. O e. the reaction is at equilibrium and the reaction will proceed at equal rates in the reverse and forward direction. Previous page os://moodle.umo.edu/mod/quiz/attempt.php?attempt3893185&cmid%3D1323382&page%=D2%#
# 4, 5, and 6
Suppose the reaction system: UO2 (s) + 4 HF (g) ← UF4 (g) + 2 H₂O (g) has already reached equilibrium. Predict the effect that each of the following changes will have on the direction of the reaction to reestablish equilibrium. Indicate whether the reaction will shift to the left, to the right, or no change. a. Additional UO2 is added to the system. b. The reaction is performed in a glass reaction container and the HF begins to react with the glass. c. Water vapor is removed. d. The pressure is increased.