1. Explain in terms of ion concentrations and Ksp why a precipitate forms for some solutions....

1. Explain in terms of ion concentrations and Ksp why a precipitate forms for some solutions.

2. When ammonia is added to a solution that has Cu(OH)2(s) precipitate in it, the precipitate dissolves. Use Le Châtelier’sprinciple to explain this.

3. Based on your observations, when a colour change occurs but no phase change occurs, what kind of reaction might have occurred?

Expert Solution

queen_honey_blossom answered 1 year ago

Give the hydronium ion and hydroxide ion concentrations of solutions with the following values of pH....

Give the hydronium ion and hydroxide ion concentrations of solutions with the following values of pH. 1. pH 13.0 for (H3O+) 2. pH 13.0 for OH- 3. pH 3.0 for H3O+ 4. pH 3.0 for OH- 5. pH 10.0 for H3O+ 6. pH 10.0 for OH-

Explain why equilibrium calculations are not necessary to determine ionic concentrations in solutions of certain strong...

Explain why equilibrium calculations are not necessary to determine ionic concentrations in solutions of certain strong electrolytes such as NaOH and HCl. Under wht conditions are equilibrium calculations necessary as part of the determination of the concentration of all ions of some other strong electrolytes in solution? (expert answer only.)

Determine whether the following hydroxide ion concentrations ([OH−]) correspond to acidic, basic, or neutral solutions by...

Determine whether the following hydroxide ion concentrations ([OH−]) correspond to acidic, basic, or neutral solutions by estimating their corresponding hydronium ion concentrations ([H3O+] using the ion product constant of water (Kw). It may help to keep the following equation in mind as you work Kw = [H3O+][OH−] = [1×10−7 M][1×10−7 M] = 1×10−14 M. 1. [OH-] = 4 x 10^-12 M 2. [OH-] = 7 x 10^-9 M 3. [OH-] = 7 x 10^-4 M 4. [OH-] = 2 x...

4. Calcium ion forms a weak 1:1 complex with nitrate ion with a formation constant of...

4. Calcium ion forms a weak 1:1 complex with nitrate ion with a formation constant of 2.0. What would the equilibrim concentrations of Ca2+ and Ca(NO3)+ in a solution prepared by adding 10.0 mL each of 0.010 M M CaCl2 and 2.0 M NaNO3? (neglect diverse ion effects). Show all work please

Propose a reason for why 2,4-DNP or semicarbazone derivatives usually precipitate out of their ethanolic solutions.

1. The following table lists the ion composition of water. What are the mg/L concentrations of...

1. The following table lists the ion composition of water. What are the mg/L concentrations of each? Does this water have charge balance? If no, then some ion is missing. Would it be a cation or an anion? From these values compute the TDS in mg/L and the hardness in mg/L as CaCO3. Are these values low, normal, or high? Is any other ion out of the desired range? Ion Concentration, mmole/L Ca2+ 4.8 Mg2+ 1.2 Fe3+ 0.5 Na+ ...

Describe how a fluoride selective ion electrode measures the fluoride ion concentration and explain why the...

Describe how a fluoride selective ion electrode measures the fluoride ion concentration and explain why the potential approaches 0 at high concentrations

(1) Identify and explain in some detail the causes for congressional gridlock and any solutions you...

(1) Identify and explain in some detail the causes for congressional gridlock and any solutions you come across in doing your research. (2) Provide at least two examples of how gridlock in recent years has prevented the passage of specific pieces of legislation intended to address one or more of our nation’s most pressing problems. These problems include infrastructure, tax reform, immigration, healthcare, entitlement reform, gun violence, income stagnation, global climate change, budget deficits, the national debt and a strong...

When Rt forms an ion, what charge would you expect it to have? Explain using quantum...

When Rt forms an ion, what charge would you expect it to have? Explain using quantum mechanics.

Describe several or some forms of cheating and why they would constitute a violation to a...

Describe several or some forms of cheating and why they would constitute a violation to a college code

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