Mg (s) + ½O2 (g) → MgO (s) (1) This equation can be obtained by combining equations (2), (3) and (4) below: MgO (s) + 2HCl (aq) → MgCl2 (aq) + H2O (l) (2) Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (g) (3) H2 (g) + ½ O2 (g) → H2O (l) (4) Combine equations (2), (3) and (4) to obtain equation (1).

What is the net ionic equation when acid HNO3 is added to base Sr(OH)2? ○ 2H3O+ (aq) + Sr(OH)2(aq) →4H2O(l) + Sr²+(aq) OH3O+(aq) + OH¯(aq) →2H2O(1) O HNO3(aq) + OH¯(aq) → H₂O(l) + NO3˜¯(aq) O 2HNO3(aq) + Sr(OH)2(aq) →2H2O(l) + Sr²+(aq) + 2NO3˜¯(aq)

Q) Drinking water may contain several unwanted ions such as phosphate ions. In order to remove the phosphate ions from the drinking water, a solution of calcium hydroxide can be added. As a result, a solid Ca5OH(PO4)3 is formed and isolated by filtration and a hydroxide ion are also formed. The reaction for this process is below: 5 Ca(OH)2 (aq) + PO43- (aq) → Ca5OH(PO4)3 (s) + OH- (aq) a) If 3.00 mL of 0.100 M calcium hydroxide is mixed with 4.00 mL of an aqueous solution of 0.0800 M phosphate ions (PO43-). What is the mass of Ca5OH(PO4)3 that can be isolated from the reaction? b) How many moles of the excess reactant remains unreacted? c) What is the concentration of the hydroxide ions in this solution? d) What is the mass of calcium (in grams) that can be recovered?

Looking up one snowy afternoon from a book titled The Moral Case Against Turning Lead Into Gold (Or Vice Versa), your friend Lena (an expert chemist) says this: "Ammonium salts heated with aqueous hydroxides form ammonia, water, and a salt." Using Lena's statement, and what you already know about chemistry, predict the products of the following reaction. Be sure your chemical equation is balanced!   NH4NO3(aq) + NaOH(aq) ->

2. What is the theoretical yield of Compound Y if you have 8.55 g of Reactant X reacted with an excess of Cr2O72? Balance the chemical equation. OH Compound X (a) OH + Cr₂O72- OH ° Compound Y OH + Cr³+ Fill in the squares in the following chemical equations: NaOH/H₂O EtOH

I need help determining which compounds will ionize.

Complete and balance the following equation: Single Replacement: 2 NaBr(aq) + Cl2(aq) →

Calculate the free energy change, AG°, for the following reaction, in kJ/mol. Report your answer to the ones place. 4Ag(s) + O2(g) + 4H*(aq)→ 4Ag*(aq) + 2H20(1I)

Write a balanced net ionic equation for each of the following acid–base reactions.   HCl(aq)+KOH(aq)→KCl(aq)+H2O(l)HCl(aq)+KOH(aq)→KCl(aq)+H2O(l) Express your answer as a net ionic equation. Identify all of the phases in your answer.