21- The mass-action effect is a shift in the position of an equilibrium caused by adding one of the reactants or products to a system. O True O False 20- Buffer solution is a mixture of a weak acid and it's salt. or weak base and it's salt. the pH of buffer resists change upon adding small amount of strong acid or base or when it dilute. O True O False 2- Equilibrium-constant are algebraic equations that describe the concentration elationships among reactants and ترك السؤال ارسال الاجابة

21- The mass-action effect is a shift in the position of an equilibrium caused by adding one of the reactants or products to a system. O True O False 20- Buffer solution is a mixture of a weak acid and it's salt. or weak base and it's salt. the pH of buffer resists change upon adding small amount of strong acid or base or when it dilute. O True O False 2- Equilibrium-constant are algebraic equations that describe the concentration elationships among reactants and ترك السؤال ارسال الاجابة

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

A solution is prepared by mixing 0.06000 mol Fe^3+ and 0.00900 mol SCN^- . It is found that 0.00800 mol of FeSCN^ 2+ exists in the solution once it reaches equilibrium. How many moles of Fe^3+ are present at equilibrium? Give answer in correct amount of significant figures.
A sample of 0.750 mol of PCl5 is heated to 250℃ in a 1.00 L reaction container to produce PCl3 and Cl2. The balanced reaction equation is PCl5(g) ßà PCl3(g) + Cl2(g) At this temperature the equilibrium constant Kc = 4.2 x 10-4. Calculate the equilibrium concentrations for PCl3 and Cl2. Use a RICE table and show all calculations. If required, check % error.
Write the equilibrium constant expression, Keq, or solubility product constant, Ksp, for each of the following reactions. COCI2 (g) → CO (g) + Cl2 (g) a. b. 2 CO2 (g) 02 (g) + 2 CO () c. AGCI (s) > Ag* (aq) + Cl (aq) d. PbCl2 (s) → Pb2* (aq) + 2 CI (aq) e. NaOH (aq) + HI (aq) <→ Nal (aq) + H20 (I)
The Solubility Product Constant for barium phosphate is 1.3 × 10-29⁹. Solid potassium phosphate is slowly added to 50.0 mL of a 0.0350 M barium acetate solution. The concentration of phosphate ion required to just initiate precipitation is
Which solution will have the lowest concentration of H* at equilibrium? 0.05 M HF (aq), K,- 6.6 x 10-4 O 0.05 M HBrO (aq), K, 2 x 10-⁹ O 0.08 M HF (aq). K₂= 6.6 x 10-4 0.08 M CH3COOH (aq). K, 1.8 x 10-5
Assume the solubility product of Mg(OH)2 is 1.3 x 10 at a certain temperature. What minimum OH concentration must be attained (for example, by adding NaOH) to decrease the Mg2+ concentration in a solution of Mg(NO3), to less than 1.2 x 10-10 M. 3/2 x 10 M (Enter your answer in scientific notation.) Next > < Prev 18 of 20 **** .*****
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 concentration of hydroxide ion, OH, in a particular solution of BrO- by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the concentration of hydroxide ion. The Kb for BrO is 4.0 × 10-6. Complete Parts 1-3 before submitting your answer. NEXT > A 0.724 M aqueous solution of BrO- was prepared. 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 4.0 x 10-6-2r 0 1 BrO (aq) 0.724 + x 0.724 0.724 - x + H₂O(l) 4.0 x 10-6 2 0.724 + 2x 0.362 0.724 - 2x OH-(aq) + HBrO(aq) +x 3 4.0 x 10-6 +x -X 4.0 x 10-6-x RESET +2x 4.0 x 10-6 + 2x
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)
Write the equilibrium constant expression, K, for the following reaction. Please enter the compounds in the order given in the reaction. If either the numerator or denominator is blank, please enter 1 K = (CH3)3N(aq) + H₂O(1) — (CH3)3 NH+ (aq) + OH¯(aq)
Fill in the left side of this equilibrium constant equation for the reaction of dimethylamine ((CH,) NH (CH,),NH). a weak base, with water. 미□
Lactase is an enzyme that breaks down the sugar lactose which is commonly found in dairy products. Some people develop lactose intolerance as they grow older and the amount of lactase enzyme in their gut diminishes. Since the enzyme is commonly found in the gut of humans it can withstand a pH that is very acidic, ranging from a pH of 2-7. A student decided to do an experiment to determine how the pH of a solution affects lactase enzyme activity. Lactase works by breaking lactose into its two component sugars of glucose and galactose. To conduct the experiment the student prepared a solution of lactose and placed it into 5 different test tubes. A pH buffer solution was then added to each test tube with a pH of 2.0 in the first tube, 4.0 in the second, 6.0 in the third, 8.0 in the fourth, and a 10 pH in the fifth. Next, the enzyme lactase was added in equal amounts to each test tube and allowed to sit for ten minutes white the enzyme reacted with the lactose. At the end of the ten…