Question

1) are solutions of potassium hypobromite, KBrO, acidic, neutral, or basic? explain using a chemical equation...

1) are solutions of potassium hypobromite, KBrO, acidic, neutral, or basic? explain using a chemical equation to demonstrate your point. 2) are solutions of ammonium iodide, NH4I, acidic, basic, or neutral? Explain using a chemical equation.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1. The pH of an aqueous solution of 0.257 M potassium nitrite, KNO2 (aq), is _____....
1. The pH of an aqueous solution of 0.257 M potassium nitrite, KNO2 (aq), is _____. This solution is (acidic, basic, neutral) 2. The pH of an aqueous solution of 0.285 M ammonium iodide, NH4I (aq), is _____. This solution is (acidic, basic, neutral)
Soluble salts containing the ammonium ion (NH4+) can give acidic, neutral or basic solutions when dissolved...
Soluble salts containing the ammonium ion (NH4+) can give acidic, neutral or basic solutions when dissolved in water. For any given salt that contains ammonium ion, describe how you would predict whether an aqueous solution of that salt would be acidic, neutral or basic. Note: Kb for the weak base, NH3, is 1.8E-5.
Determine if the following salt solutions (0.123 M) are basic, acidic or neutral. Determine the pH...
Determine if the following salt solutions (0.123 M) are basic, acidic or neutral. Determine the pH of the solution, if possible. (Ammonium: Ka = 5.8 x 10-10, Sulfate: Kb = 8.3 x 10-13) a. Sodium nitrate b. Sodium sulfate c. Ammonium nitrate d. Ammonium sulfate
1. The pH of an aqueous solution of 0.285 M ammonium iodide, NH4I (aq), is _____....
1. The pH of an aqueous solution of 0.285 M ammonium iodide, NH4I (aq), is _____. This solution is (acidic, basic, neutral)
State whether each of the following aqueous solutions would be acidic, basic, or neutral and explain...
State whether each of the following aqueous solutions would be acidic, basic, or neutral and explain your answer. Include the appropriate net-ionic equations to show why a given solution is acidic or basic. Use Ka or Kb values if needed. a. HCO2H b. 50:50 mixture of HCO2H + NaHCO2 c. ((CH3)2NH2)Cl d. 50:50 mixture of (CH3)2)NH + ((CH3)2NH2)Cl
Determine whether aqueous solutions of the following salts are acidic, basic, or neutral. (a) MgC2O4 acidicbasic    neutral...
Determine whether aqueous solutions of the following salts are acidic, basic, or neutral. (a) MgC2O4 acidicbasic    neutral (b) C5H5NHCl acidicbasic    neutral (c) CrCl3 acidicbasic    neutral (d) CsClO4 acidicbasic    neutral
Decide if aqueous solutions of the following are acidic, basic, or neutral. For each, write the...
Decide if aqueous solutions of the following are acidic, basic, or neutral. For each, write the balanced equation that determines the pH of the solution. All species should include charge (if any) and phase. On the product side, list the cation (if any) first, followed by the neutral molecule (if any), and the anion (if any). (See Appendix E for K values.) Ba(NO3)2 Solution is: Li2CO3 Solution is: (CH3)3NHBr Solution is: NaCH3CO2 Solution is:
State whether each of the following aqueous solutions would be acidic, basic, or neutral and explain...
State whether each of the following aqueous solutions would be acidic, basic, or neutral and explain your answer. Include the appropriate net-ionic equations to show why a given solution is acidic or basic. (Use your text to look up Ka or Kb values if needed. HCO2H = formic acid; (CH3)2 = dimethyl amine.) A. KCl B. HCO2H C. 50:50 mixture of HCO2H + NaHCO2 D. ((CH3)2NH2)Cl E. 50:50 mixture of (CH3)2NH + ((CH3)2NH2)Cl F. 50:50 mixture of 0.1 M NaNO3...
1) Is the solution of C5H5NHClO4 acidic, basic or neutral? 2) Is the solution of NH4NO2...
1) Is the solution of C5H5NHClO4 acidic, basic or neutral? 2) Is the solution of NH4NO2 acidic, basic or neutral? 3) Is the solution of NH4F acidic, basic or neutral? 4) Is the solution of CH3NH3CN acidic, basic or neutral?
1) Write the net ionic equation for the equilibrium that is established when ammonium iodide is...
1) Write the net ionic equation for the equilibrium that is established when ammonium iodide is dissolved in water. (Use H3O+ instead of H+.) This solution is acidic, basic or neutral? 2)Write the net ionic equation for the equilibrium that is established when calcium nitrite is dissolved in water. The solution is acidic, basic or neutral? 3)Write the net ionic equation for the equilibrium that is established when barium cyanide is dissolved in water. This solution is acidic, basic or...