i. Write the net ionic equation for the equilibrium involving the HSO HSO ) + H2O...

Question

Question

Answer 1

Answer #1

i. H₂SO_4(aq) + H₂O_(l) $\rightleftharpoons$ HSO₄^-_(aq) + H₃O⁺_(aq)

HSO₄^-_(aq) +H₂O_(l) $\rightleftharpoons$ SO₄²^-_(aq) + H₃O⁺_(aq)

vii.

H₂SO_4(aq) + H₂O_(l) $\rightleftharpoons$ HSO₄^-_(aq) + H₃O⁺_(aq) + heat

HSO₄^-_(aq) +H₂O_(l) $\rightleftharpoons$ SO₄²^-_(aq) + H₃O⁺_(aq) + heat

Answer 2

Similar Homework Help Questions

a.Write the net ionic equation for the equilibrium that is established when ammonium perchlorate is dissolved...

a.Write the net ionic equation for the equilibrium that is established when ammonium perchlorate is dissolved in water. It is not necessary to include states such as (aq) or (l). + H2O + This solution is _________acidicbasicneutral b.Write the net ionic equation for the equilibrium that is established when calcium hypochlorite is dissolved in water. It is not necessary to include states such as (aq) or (l). + H2O + This solution is _________acidicbasicneutral
For the chemical reaction HClO4(aq)+NaOH(aq)⟶H2O(l)+NaClO4(aq) write the net ionic equation, including the phases. net ionic equation:

For the chemical reaction HClO4(aq)+NaOH(aq)⟶H2O(l)+NaClO4(aq) write the net ionic equation, including the phases. net ionic equation:
2) Day 18 & MQ16: Write the balanced net ionic equation for the following cells in...

2) Day 18 & MQ16: Write the balanced net ionic equation for the following cells in acidic conditions: a. Cr(s) Cr" (aq) || Re" (aq)| Re(s) _Reacaq) +cres) _Rels) + _crofag) b. Pt() | H2O(1),02(g) || Cu?*(aq) Cu(s) - Ptest Cu 2+ cag) H2011) + Oziq) + Cu(s)

Write the net ionic equation for: HF (aq)+NaOH (aq)→NaF (aq)+H2O (l)

Write the net ionic equation for: HF (aq)+NaOH (aq)→NaF (aq)+H2O (l)
(1) Write a net ionic equation for the reaction between HSO3 and CH3COOH that shows HSO;...

(1) Write a net ionic equation for the reaction between HSO3 and CH3COOH that shows HSO; behaving as a Bronsted-Lowry base. Use CH3COOH for acetic acid and CH C00 for the acetate ion. (Use the lowest possible coefficients. Omit states of matter.) BL base BL acid BL acid BL base + + (2) Decide which would be favored at equilibrium for this reaction, reactants or products? Submit Answer Retry Entire Group 9 more group attempts remaining
Write the following as a net ionic equation: HCl(aq) + H2O(l) → H3O+(aq) + Cl −(aq)

Write the following as a net ionic equation: HCl(aq) + H2O(l) → H3O+(aq) + Cl −(aq)

3. A student is studying the equilibrium described by the net ionic equation shown in Equation...

3. A student is studying the equilibrium described by the net ionic equation shown in Equation 18. 2+ U) (Eq. 18) (1) The student adds sodium bromide solution (NaBr) to a sample of the blue equilibrium mixture in or- der to increase the Br ion concentration. Predict what the student will observe, and explain your prediction. CuBr4(aq, green) +6 H2O
Write a balanced net ionic equation for the following reaction in basic solution using H2O method...

Write a balanced net ionic equation for the following reaction in basic solution using H2O method for balancing a redox reaction: MnO4-(aq) + C2H5OH(aq) → Mn2+(aq) + HC2H3O2 (aq)
33 Write the net ionic equation for the acid-base hydrolysis equilibrium that is established when sodium...

33 Write the net ionic equation for the acid-base hydrolysis equilibrium that is established when sodium nitrite is dissolved in water. + H2O(0) = This solution is Write the net ionic equation for the acid-base hydrolysis equilibrium that is established when calcium hypochlorite is dissolved in water + H20(0) = This solution is

Write the net ionic equation for the acid-base hydrolysis equilibrium that is established when potassium cyanide...

Write the net ionic equation for the acid-base hydrolysis equilibrium that is established when potassium cyanide is dissolved in water. + H2O(l) = This solution is Submit Answer Retry Entire Group 8 more group attempts remaining The pH of an aqueous solution of 0.200 M ammonium perchlorate, NH_CI04 (aq), is . This solution is - Submit Answer Retry Entire Group 9 more group attempts remaining