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Write a balanced chemical equation (including phases) to describe the following reactions of sulfuric acid and...
Write a balanced chemical equation (including phases) to describe the following reactions of sulfuric acid and nitric acid: Nitric acid reacts with ammonia in aqueous solution. HNO_3(aq) + NH_3(aq) implies NH^+_4(aq) + NO^-_3(aq) Sulfuric acid reacts with ammonia in aqueous solution. H_2SO_4(aq) + 2 NH_3(g) implies (NH_4)_2 SO_4(aq) Sulfuric acid dissolves in water. Step 1 (1st proton): H_2SO_4(aq) + H_2O(l) implies H_3O^+(aq) + HSO^-_4(aq) Step 2 (2nd proton): HSO^-_4(aq) + H_2O(l) implies H_3O^+(aq) + SO^2-_4(aq)
Write the balanced chemical equation for all the reactions. Please include phases 1) Aqueous (NH4)3PO4 reacts with aqueous MgBr2 2) Gaseous C2H8 reacts with elemental oxygen 3) Aqueous HCl reacts with aqueous Na2CO3 4) Aqueous LiOh reacts with aqueous Na2SO4
or H mple Exercise 7.16: Neutralization Reactions Part A Write a balanced chemical equation for the following neutralization reaction producing a soluble sa Bromic acid, HBrOs, neutralizes an ammonium hydroxide solution. Express your answer as a chemical equation including phases. View Available Hint(s) Xa Xb bb x →: .@白 . Submit Incorrect, Try Again: 7 attempts remaining Part B Write a balanced chemical equation for the following neutralization reaction producing a soluble salt Hydrocyanic acid, HCN neutralizes a calcium hydroxide...
6. Write a balanced equation describing each of the following chemical reactions. (a) Solid potassium chlorate, KClO3, decomposes to form solid potassium chloride and diatomic oxygen gas. (b) Solid aluminum metal reacts with solid diatomic iodine to form solid Al2I6. (c) When solid sodium chloride is added to aqueous sulfuric acid, hydrogen chloride gas and aqueous sodium sulfate are produced. (d) Aqueous solutions of phosphoric acid and potassium hydroxide react to produce aqueous potassium dihydrogen phosphate and liquid water.
Write the balanced chemical equation for each of these reactions. Include phases. When aqueous sodium hydroxide is added to a solution containing lead nitrate, a solid precipitate forms. However, when additional aqueous hydroxide is added the precipitate redissolves forming a soluble [Pb(OH)_4]^2- (aq) complex ion.
Predict the products and write a balanced chemical equation for each of the filling problems. Include phases ( g,s,l,aq) thank you. If there is no reaction write no rxn ( please ignore my pencil and red pen marks ) 4. Predict the products and write a balanced chemical equation for the following reactions reaction does not occur, writer NO RXN. For full credit include phases!ll (10 Points a. Aqueous NaOH reacts with aqueous FeBr3: b. Gaseous CaHe reacts with elemental...
Write the balanced chemical equation for each of the reactions. Include phases. When aqueous sodium hydroxide is added to a solution containing lead(II) nitrate, a solid precipitate forms. equation: However, when additional aqueous hydroxide is added, the precipitate redissolves, forming a soluble [Pb(OH)4]2−(aq)[Pb(OH)4]2−(aq) complex ion. equation:
Write balanced ionic equations for the following reactions: Aqueous hydrobromic acid is neutralized by aqueous calcium hydroxide. Express your answer as a full ionic equation. Identify all of the phases in your answer. Aqueous potassium hydroxide is neutralized by aqueous sulfuric acid. Express your answer as a full ionic equation. Identify all of the phases in your answer.
write a balanced equation including phases, and identifying the chemical formula of the precipitate. Part 1 - Preparation of CaCO3(s) The following is a procedure that was theoretically performed by a student. Read through the procedure and answer the questions below. 1. A 10.0 mL graduated cylinder to measure 10.0 mL of a 1.00 M CaCl2 solution into an initially empty 50.0 mL beaker. 2. A 50.0 ml graduated cylinder was then used to measure out 25.0 mL of 0.500...
Write the balanced chemical equation for each of the reactions. Include phases. When aqueous sodium hydroxide is added to a solution containing lead(II) nitrate, a solid precipitate forms. equation: 2 NaOH + Pb(NO3)2 + Pb(OH), + 2NaNO, However, when additional aqueous hydroxide is added, the precipitate redissolves, forming a soluble (Pb(OH),12- (aq) complex ion. equation: Pb(OH), +20H (Pb(OH) 2 -