Explain why we can simplify the calculations for K when the value of K is very small (less than ~104). 4.1 4.2 HCN will react very slightly with water with a K = 6.2 x 1010. HCN(aq) + H,O() H,O* (aq) and CN¯ (aq) A chemist starts with a 0.50 M HCN solution. What is the equilibrium concentration of H;O*?. Then use the concentration of H3O* to calculate the pH of the solution with the equation pH = -log[H,O*] (you can do this!!!). Put your final answers in the box. If you need more space to show your work, Nou can use the backside of this page. %3D [H,O'] at equilibrium M pH = -log[H,O*] pH = % of HCN that reacted

Explain why we can simplify the calculations for K when the value of K is very small (less than ~104). 4.1 4.2 HCN will react very slightly with water with a K = 6.2 x 1010. HCN(aq) + H,O() H,O* (aq) and CN¯ (aq) A chemist starts with a 0.50 M HCN solution. What is the equilibrium concentration of H;O?. Then use the concentration of H3O to calculate the pH of the solution with the equation pH = -log[H,O] (you can do this!!!). Put your final answers in the box. If you need more space to show your work, Nou can use the backside of this page. %3D [H,O'] at equilibrium M pH = -log[H,O] pH = % of HCN that reacted

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

Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 3 > A solution is prepared with 0.55 M HNO2 and 0.75 M KNO2. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -2x 0.75 -2x 0 1 HNO₂(aq) 0.55 + x 0.55 -X 0.55-x 0.55 0.55 - x 0.75 2 H₂O(l) III 0.55 + 2x 6.8 x 104 0.55 - 2x 1L +x H3O+(aq) 0.75 + x +x -X 0.75-x + NO₂ (aq) RESET +2x NEXT 0.75 + 2x +x
1) Write the equilibrium expression for the solid calcium hydroxide and the dissolved ions. A saturated, aqueous, solution of Ca(OH)2 equation: Ca(OH)2 (s) ↔ Ca2+ (aq) + 2OH– (aq) The equilibrium expression for calcium hydroxide: Ksp = [Ca2+][OH–]2
Consider the following reaction:  Ag+ (ag) + 2 NH3 (aq) = Ag(NH3)2+ (aq) Keq = 7.99 An initial concentration of Ag+ = 0.0100 M was combined with NH3 and allowed to reach equilibrium. If the equilibrium concentration of Ag(NH3)2+= 0.00278 M, What was the initial concentration of NH3?
Given the two reactions 3. PbCl 2 (aq)⇌Pb 2+ (aq)+2Cl − (aq), K 3 = 1.80×10−10, and4. AgCl(aq)⇌Ag + (aq)+Cl − (aq), K 4 = 1.13×10−4,what is the equilibrium constant K final for the following reaction?PbCl 2 (aq)+2Ag + (aq)⇌2AgCl(aq)+Pb 2+ (aq)
A 0.050 M solution of the salt NaA has a pH of 9.00. Determine the [OH] and the pH of a 0.010 M solution of the acid HA. Show your work in the question parts below. Construct an ICE table for the ionization equation described below.. Use the given information to determine the concentration at equilibrium for all reactants and products.. Initial () Change () Equilibrium () 0.050 + x 0.050 + 2x A (aq) 0 0.050- x A (aq) + H₂O(1) HA(aq) + OH(aq) 0.050 - 2x + 0.050 0.100 + x 0.100 + 2x 0.100 0.100 - x H₂O(l) 0.100 - 2x -X (0.050 + x)² = +x (0.050- x)² +2x HA(aq) (0.100 + x)² RESET -2x (0.100 - x)² + OH (aq)
0.030 moles of a weak acid, HA, was dissolved in 2.0L of water to form a solution. At equilibrium, the concentration of HA was found to be 0.013 M. Determine the value of Ka for the weak acid. 1 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. HA(aq) H20(1) H3Oʻ(aq) A (aq) + + Initial (M) Change (M) Equilibrium (M)
0.030 moles of a weak acid, HA, was dissolved in 2.0 L of water to form a solution. At equilibrium, the concentration of HA was found to be 0.013 M. Determine the value of Ka for the weak acid. 1 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. H¿O(I) H.O*(aq) A (aq) + НА(ag) Initial (M) Change (M) Equilibrium (M) 5 RESET 0.060 0.015 0.017 0.030 0.013 2.0 8 2/ pe here to search DELL 1L
Determine the pOH of a weak acid (HA) solution by constructing an ICE table and using this information to determine the pOH of the solution. Complete Parts 1-2 before submitting your answer. 1 A 0.200 M aqueous solution of HA is 3.0% dissociated at equilibrium. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) HA(aq) + H₂O(l) 2 H3O+ (aq) 2 NEXT > + A-(aq)
In a lab experiment, a student manages to dissolve 0.00250 moles of a mysterious compound AB into 1 L of water. The mysterious compound dissociates using the following equation: AB(S) ⇌ A(aq) + B(aq) What is the value of the Ksp for this compound? (Please provide your answer to 3 significant figures in scientific notation such as 1.23*10^-5.)
Given a solution whose equation is expressed below, identify the (a) shift in equilibrium (b) effect on the concentration of the chloride ion (c) effect on the equilibrium constant when the solution is diluted with water. CoCl4^2- + 6H2O = Co(H2O)6^2+ +4Cl^-
The questions below refer to the following system: Co(H2O)6 + 4 CI=C0C1 + 6H,O (pink) (blue) When cobalt(II) chloride is added to pure water, the Co-" ions hydrate. The hydrated form then reacts with the Cl ions to set up the equilibrium shown here. Which statement below describes the change that the system will undergo if water is added? Select one: O a. More chloride ions will be produced. O b. The equilibrium will shift to the right. O c. There will be less of the hydrated cobalt ion at the new equilibrium position. O d. More water will be produced. O e. The color will become more blue. here to search F4 F6 F7 F8 F10 F11 F12 Prisc %23 %24 & 4. 5 6 E R T G B
At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The resulting equilibrium solution has a pH of 10.16. What is the Ksp of the salt at 22 °C? KsP