Measured pH of the solution: Calculate the H₂O* at equilibrium for this solution (include units): pH - log(H30+) H30 + = 10"H H30 + = 10 [H0]=,M Show work: 3. Calculate the C₂H₂O₂at equilibrium for this solution (include units): [C₂H302] = M Show work: 4. What is the HC,H,0₂ at equilibrium for this solution(include units)? [HC₂H₂O₂] = M Show work: Calculate K and pK for this solution: Determination of Ka was used of 10.0ml of 1.0 M acetic acid into a beaker and the pH was 2.22 0 3 a a

can you help me how to write the appropriate equilibrium equation for the acid can you please put the STATE OF MATTER TO, CAN YOU PLEASE PUT THE SIGNS TOO? HONH3NO3

t Given the following equilibrium constants at 437°C, K₁ = 3 × 10-25 K₂ = 1 x 10-5 K3 = 9 × 10-29 K4 = 4 x 10-14 [References] Na₂O(s) = 2 Na(l) + O2(g) NaO(g) ⇒ Na(1) + 0₂ (9) 2 Na2O2 (s) 2 Na(l) + O₂(g) NaO₂ (s) Na(l) + O2(g) determine the values for the equilibrium constants for the following reactions: a. Na₂0(8) + 0₂ (9) ⇒ Na₂O₂ (s) Equilibrium constant = b. NaO(g) + Na2O(s) ⇒ Na₂O₂ (s) + Na(1) Equilibrium constant = c. 2 NaO(g) Na₂O₂ (s) Equilibrium constant = (Hint: When reaction equations are added, the equilibrium expressions are multiplied.) Submit Answer 6 item attempts remaining Try Another Version Show Hint Previous Next

Predict the signs of delta H for the reaction below: (HINT: H is the same as potential energy. Low --> High (delta is positive) and High > Low (delta is negative). P (s) + 6 H₂(g) --> 4 PH₂(g) AH0 Exothermic AH> 0 Endothermic OAH < 0 Endothermic

Initially 3.0 mol of nitrosyl bromide NOBr is placed in a 5.0L container and allowed to come to equilibrium at 25°C. If the nitrosyl bromide is 12% dissociated, calculate Kc 2NOBr (= sign) 2NO + Br2

part c please

7 8 9 6 Submit Tap here or pull up for additional resources 个 10 (aq) O H H₂O

The following equilibrium constants have been determined for hydrosulfuric acid at 25°C: H2S(aq) = H*(aq) + HS (aq) K¸' = 9.5 × 10-8 HS (aq) = H*(aq) + S²¯(aq) K¸" = 1.0 × 10-19 es Calculate the equilibrium constant for the following reaction at the same temperature: H,S(aq) = 2H*(aq) + s²¯(aq) K = x 10

What is the equilibrium constant expression for the following reaction: NH4+(aq) + Cl−(aq)↔NH4Cl(s) Choose from the list below and enter the letters alphabetical order. (e.g. For an equilibrium constant of [Cl-]2eq[NH4+]eq enter AH.)

Please calculate the Ka for a weak acid given the following data: pH = 3.72, and an initial acid concentration of 1.43 x 10-4 M (note: please express your answer with 3 sig figs.; the equilibrium reaction is shown below:) НА(аq) + H,0 () H;O* (aq) + A´ (: