Can you please help me with d, e, f, and g? NAMEPER2. Suppose a 0.0500M solution of HNO, was createdWrite the dissociation reaction for this compound. (use correct symbols)a.HNO3 (aq)+H20(1)→ H(aq) + NO5 (aq)b. Write the equilibrium expression for the acid dissociation constant, K for this acid:(H+][NO5]し、(H20)(HNO,]c. Calculate the [H'] concentration at equilibrium at a temperature where its K, is equal to 4.5 x 10sしa(H+][NO3]0.0600-X X 0.DS00[H20][HND;]4.5 x10-5=X= J4.5 x10-5X0.05000.0500 -X4.5x 10-5=x20,0500d. Calculate the pH at equilibrium at this temperature.Calculate the percent dissociation of HNO, at equilibrium at this temperature. Also answer this: If youwere to dilute this solution the percent dissociation would [increase; decrease].e.CENGAGELearning AP® EDITONNAMEPERf. In a separate beaker, 5.00 grams of KNO,(1) are dissolved in water to make a 500, mL solution.Calculate the initial molar concentration of NO, ions.ii.Calculate the K, for NO, at this temperature. Assume K, is still equal to 1014 at this temperature.ii.Calculate the pH of this solution.At 25°C, the K of HNO, = 4.0 x 104. If the overall process of the dissociation of the acid is exothermic,was the temperature originally suggested (in part c) higher or lower than 25°C. Justify your response.

d.Given, 0.0500M HNO3 solution with Ka value 4.5×10-5. What is the value of pH?

c. Calculate the [H'] concentration at equilibrium at a temperature where its K, is equal to 4.5 x 10 (H)N03] [H20][HNO,] 0.0600-X x 0.0S00 %3D 4.5x10-5= x= J4.5 KI0-6X0.0500 0.0500 -x X=1,5 K10-3 2. 4.5x 10-5= 0,0500 d. Calculate the pH at equilibrium at this temperature. e. Calculate the percent dissociation of HNO, at equilibrium at this temperature. Also answer this: If ye were to dilute this solution the percent dissociation would [increase; decrease].

c. Calculate the [H'] concentration at equilibrium at a temperature where its K, is equal to 4.5 x 10 (H)N03] [H20][HNO,] 0.0600-X x 0.0S00 %3D 4.5x10-5= x= J4.5 KI0-6X0.0500 0.0500 -x X=1,5 K10-3 2. 4.5x 10-5= 0,0500 d. Calculate the pH at equilibrium at this temperature. e. Calculate the percent dissociation of HNO, at equilibrium at this temperature. Also answer this: If ye were to dilute this solution the percent dissociation would [increase; decrease].

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.11PAE

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