Homework Answers
1) The higher the acid Ka, the greater the acidity force and the lower pH, then the second lower pH is that of HF, Option D.
2) Option C. When equilibrium is reached, the concentrations of the substances do not change.
3) Kp is calculated:
Kp = Kc * (R * T) ^ Δn = 3.64x10 ^ -3 * (0.082 * 298) ^ (2-1) = 8.9x10 ^ -2
Option B.
4) The expression of equilibrium is:
K = [CO] ^ 2 / [CO2]
Option D.
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DIRECTIONS: A COMPLETE THE ANSWER SHEET: Write your name. banner id # and the...
answer all 6) cernents is true? equilibrium co the right 5) Determine the value of Ke...
answer all
6) cernents is true? equilibrium co the right 5) Determine the value of Ke for the following reaction if the equilibrium concentrations are as follows: (NO Joy -0.85 M and [NO_Jeg -0.38 M. 2 NO:(8) - N,Od D) 0.22 E) 0.53 A) 2.2 C) 0.022 B) 19 6) Which of the following statements is true? A) 10-K, it means the reaction is not at equilibrium. B) TOK, it means the forward reaction will proceed to the right to...
5) Determine the value of Kc for the following reaction if the equilibrium concentrations are as...
5) Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [NO2]eq = 0.85 M and [NO]eq=0.38 M. 2 NO2(g) - N2048) A) 2.2 B) 1.9 C) 0.022 D) 0.22 E) 0.53 6) Which of the following statements is true? A) If Q=K, it means the reaction is not at equilibrium. B) If Q<K, it means the forward reaction will proceed to the right) to form more reactants. C) IFO <K, it means the...
6) Which of the following statements is true? A) If Q = K, it means the reaction is not at equilibrium B) If Q<...
6) Which of the following statements is true? A) If Q = K, it means the reaction is not at equilibrium B) If Q< K, it means the forward reaction will proceed (to the right) to form more reactants. C) If Q< K, it means the reverse reaction will proceed (to the left) to form more reactants. D) If Q> K, it means the forward reaction will proceed (to the right) to form more reactants E) If Q> K, it...
R-0.08206 (atm - L)(mol - K)= 8.314 J/(mol-K) pH = -log[H30) pOH = -log(OH) pX=-logX [HO'] = 10 Ph. K, EK.(RT) pH +...
R-0.08206 (atm - L)(mol - K)= 8.314 J/(mol-K) pH = -log[H30) pOH = -log(OH) pX=-logX [HO'] = 10 Ph. K, EK.(RT) pH + pOH = 14 = pK+pKb [OH (H:0= 10-14 = K, * Ks (in water at 25°C) pH =pK, + log([base)/(acid]) pOH =pKy + log (acid]/[base]) Molar Solubility = (*+ m for a salt that dissociates into ions with coefficients of n and m - b b -4ac where 0 = ax + bx+c VA= A/ X=- 1)...
When dealing with buffer systems, we often use the acid reaction to determine the equilibrium and...
When dealing with buffer systems, we often use the acid reaction to determine the equilibrium and set up the ICE table. The most common experimental method used to study acid-base systems is titration, which studies the stoichiometric addition of the acid to a base solution or the base to an acid solution to determine the value of K, or K, The value of the pK, or pK, is essential to the understanding of the buffer system, where pK, = -log...
Question two A buffer solution is able to maintain a constant pH when small amounts of...
Question two
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 ml solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O2. The initial concentration of both the acid and the base are 0.0100 mol/0.1000...
A buffer solution is able to maintain a constant pH when small amounts of acid or...
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
Instructions: Complete all the problems in this assignment Show all your work and submit a PDF...
Instructions: Complete all the problems in this assignment Show all your work and submit a PDF with your answers through Husky CT for your lab section. Please e-mail me if you have an issues with the submission. Activity #1 Calculate the pH for the following acidic solutions 1. Calculate the pH and pOH for the following solutions: a. 0.200 M HNO3 b. 0.200 M H2SO4 2. Calculate the equilibrium concentration for [H], [A-], and [HA], the pH and pOH for...
In the following questions write your answers with the detailed steps. Show all necessary equations or...
In the following questions write your answers with the detailed steps. Show all necessary equations or conversion factors. a. 4.50 g sample of glucose (C6H12O6) is dissolved in enough water to make 10.0 mL of solution. Calculate the molarity. b. 424 g of solute is dissolved in enough water to give 1.00 L of solution. The density of the resulting solution is 1.18 g/mL. What is the %(w/w)? c. Write a reaction equation that corresponds to the following equilibrium expression:...
CHM1046L, Quiz 4 Practice, Exp. 9 --- Show all work with units. Equations: pH = -log[1],...
CHM1046L, Quiz 4 Practice, Exp. 9 --- Show all work with units. Equations: pH = -log[1], pH + pOH = 14, pH = pka + log HA 1. The concentration of HNO, is 1 M, calculate its pH and pOH. 2. The concentration of NaOH is 10 M, calculate its pOH and pH. Suppose a buffer (PK, - 4) contained 5 moles of HA and 5 moles of A, calculate the pH when: A. 1 mole of HCl is added....
answer all
6) cernents is true? equilibrium co the right 5) Determine the value of Ke for the following reaction if the equilibrium concentrations are as follows: (NO Joy -0.85 M and [NO_Jeg -0.38 M. 2 NO:(8) - N,Od D) 0.22 E) 0.53 A) 2.2 C) 0.022 B) 19 6) Which of the following statements is true? A) 10-K, it means the reaction is not at equilibrium. B) TOK, it means the forward reaction will proceed to the right to...
5) Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [NO2]eq = 0.85 M and [NO]eq=0.38 M. 2 NO2(g) - N2048) A) 2.2 B) 1.9 C) 0.022 D) 0.22 E) 0.53 6) Which of the following statements is true? A) If Q=K, it means the reaction is not at equilibrium. B) If Q<K, it means the forward reaction will proceed to the right) to form more reactants. C) IFO <K, it means the...
6) Which of the following statements is true? A) If Q = K, it means the reaction is not at equilibrium B) If Q< K, it means the forward reaction will proceed (to the right) to form more reactants. C) If Q< K, it means the reverse reaction will proceed (to the left) to form more reactants. D) If Q> K, it means the forward reaction will proceed (to the right) to form more reactants E) If Q> K, it...
R-0.08206 (atm - L)(mol - K)= 8.314 J/(mol-K) pH = -log[H30) pOH = -log(OH) pX=-logX [HO'] = 10 Ph. K, EK.(RT) pH + pOH = 14 = pK+pKb [OH (H:0= 10-14 = K, * Ks (in water at 25°C) pH =pK, + log([base)/(acid]) pOH =pKy + log (acid]/[base]) Molar Solubility = (*+ m for a salt that dissociates into ions with coefficients of n and m - b b -4ac where 0 = ax + bx+c VA= A/ X=- 1)...
When dealing with buffer systems, we often use the acid reaction to determine the equilibrium and set up the ICE table. The most common experimental method used to study acid-base systems is titration, which studies the stoichiometric addition of the acid to a base solution or the base to an acid solution to determine the value of K, or K, The value of the pK, or pK, is essential to the understanding of the buffer system, where pK, = -log...
Question two
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 ml solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O2. The initial concentration of both the acid and the base are 0.0100 mol/0.1000...
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
Instructions: Complete all the problems in this assignment Show all your work and submit a PDF with your answers through Husky CT for your lab section. Please e-mail me if you have an issues with the submission. Activity #1 Calculate the pH for the following acidic solutions 1. Calculate the pH and pOH for the following solutions: a. 0.200 M HNO3 b. 0.200 M H2SO4 2. Calculate the equilibrium concentration for [H], [A-], and [HA], the pH and pOH for...
In the following questions write your answers with the detailed steps. Show all necessary equations or conversion factors. a. 4.50 g sample of glucose (C6H12O6) is dissolved in enough water to make 10.0 mL of solution. Calculate the molarity. b. 424 g of solute is dissolved in enough water to give 1.00 L of solution. The density of the resulting solution is 1.18 g/mL. What is the %(w/w)? c. Write a reaction equation that corresponds to the following equilibrium expression:...
CHM1046L, Quiz 4 Practice, Exp. 9 --- Show all work with units. Equations: pH = -log[1], pH + pOH = 14, pH = pka + log HA 1. The concentration of HNO, is 1 M, calculate its pH and pOH. 2. The concentration of NaOH is 10 M, calculate its pOH and pH. Suppose a buffer (PK, - 4) contained 5 moles of HA and 5 moles of A, calculate the pH when: A. 1 mole of HCl is added....
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