11)
Given:
pOH = 3.65
use:
pOH = -log [OH-]
3.65 = -log [OH-]
[OH-] = 2.239*10^-4 M
Answer: 2.24*10^-4 M
12)
Given:
pOH = 6.87
use:
pOH = -log [OH-]
6.87 = -log [OH-]
[OH-] = 1.35*10^-7 M
Answer: 1.35*10^-7 M
#11/12 8. [H3O+] = 4.3 x 10-3M Instructions: Calculate the [H3O+] of solutions a and b;...
Instructions: Determine if each solution is acidic, basic, or neutral. [H3O+] = 1 x 10-10 M; [OH-] = 1 x 10-4 M [H3O+] = 1 x 10-7 M; [OH-] = 1 x 10-7 M [H3O+] = 1 x 10-1 M; [OH-] = 1 x 10-13 M [H3O+] = 1 x 10-13 M; [OH-] = 1 x 10-1 M Instructions: Calculate [OH-] given [H3O+] in each aqueous solution and classify the solution as acidic or basic. [H3O+] = 2.6 x 10-3...
#2 10. PH - 3.65 11. pOH = 3.65 2. 1 12. POH = 6.87 [1.35.10T-7. Equilibrium and Le Chateleir's Principal Instructions: Write the equilibrium expression for each chemical equation 1. 2 H256) = 2H2(g) +526), K=2H2 - LH₂5 2. NH_HS(9) = NH3(g) + H250g) Oxidation-Reduction Reactions Instructions: Assign an oxidation state to each element, ion, or mole 1. C = 2. Br2 Glidaten t o
Calculate the pH and pOH of each of the following solutions. [H3O+]= 1.5×10−8 M [H3O+]= 1.0×10−7 M [H3O+]= 2.1×10−6 M
Calculate the pH and pOH of each of the following solutions. Part A [H3O+]= 1.5×10−8 M Express your answer to two decimal places. Enter your answers numerically separated by a comma. pH, pOH = Part B [H3O+]= 1.0×10−7 M Express your answer to two decimal places. Enter your answers numerically separated by a comma. pH, pOH = Part C [H3O+]= 2.5×10−6 M Express your answer to two decimal places. Enter your answers numerically separated by a comma. pH, pOH =
For the following reaction, calculate how many moles of NO2 forms when 0.356 moles of the reactant completely reacts. 2 N2O5g→4 NO2g+O2g For the following reaction, calculate how many moles of each product are formed when 0.356 moles of PbS completely react. Assume there is an excess of oxygen. 2PbSs+3O2g→2PbOs+2SO2g For the following reaction, calculate how many grams of each product are formed when 4.05 g of water is used. 2 H2O→2 H2+O2 4. Determine the theoretical yield of P2O5,...
11. Calculate pH of the following solutions. At 25°C, Kw- [H30*] [OH'] = 1.00 x 10-14 pH=-log [H30 ] a) [H30 ] 2.30 x 10-12 M pOH=- log [OH] pH+ pOH = 14 b) [OH]=9.7x 102 M
2. Calculate the pH of the following solutions: (a) [H3O+] = 1.4 x 10-'M (b) [OH-] = 3.5 x 10-2M (c) pOH = 10.5 3. What is the pH of a 0.10 M solution of HCIO4? (A strong acid) 4. Write the dissociation reaction and the corresponding K, expression for the following acids in water. (a) H3PO4 (b) C&H OH 5. Write the reaction and corresponding Ko expression for each of the following bases in water. (a) NH3 (b) PO4...
Can anyone please help with how to calculate degree of ionization for the first 3 solutions as well as how to calculate the expected pH for solution 4? thank you! Experiment 8: Equilibria of Weak Acids and Bases Lab Report Sheet 1 Composition 20.0 mL of 0.1 M HC2H302 - (A weak acid) pH 12.76 2.42 2.59 10.0 mL of 0.10 M HC2H3O2 + 10.0 mL H20 - (effect of dilution on the degree of ionization of weak acid) 10.0...