1. Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, write only NR. Ba(CHO₂)₂
2. Write the formula of the conjugate base of the Brønsted-Lowry acid, HC₂O₄⁻
3. What is the pH of a 0.0880 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?
4. What is the pH of a 0.600 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
1. Determine if the following salt is neutral, acidic or basic. If acidic or basic, write...
Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilbirium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, write only NR. CH3NH3CI
Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilbirium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, write only NR. LiCNO
Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, write only NR. CaCl₂
Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilbirium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, write only NR. CH3NH3CI
1. Write the equilibrium expression for the autoionization of water. Using this expression define the terms acid and base and pH. 2. Calculate the pH, pOH, Ka, Kb, pKa, and pKb for a 0.082M solution of triethylamine. 3. Calculate the pH, pOH, Ka, Kb, pKa, and pKb for a 1.570 M solution of hydrogen cyanide. 4. The acid-dissociation constant for hypochlorus acid is 3.0 X 10-8. Calculate the concentrations of H3O+, CIO-, and HCIO at equilibrium if the initial concentration...
Indicate whether each of the following compounds will give an acidic, basic or neutral solution when dissolved in water. Clear All ammonium chloride The pH will be less than calcium nitrite The pH will be approximately equal to 7 potassium nitrate The pH will be greater than 7 ammonium nitrate For the following reaction, the reactants are favored at equilibrium. Classify each of the reactants and products based on their strength as Bronsted-Lowry acids or bases. CIO+CHINHCH N + HCIO...
please help >< Polyprotic acids have more than one proton to donate to water, therefore have more than one equilibrium constant for proton donation. For phosphoric acid, there is a three-step equilibrium: H, PO +H,0 5 H2PO4 + H30* H,PO," +H,0 5 HPO - +H30* HPO 2- +,0 5 PO.- +,0* Kai = 7.11 x 10-3 Ka2 = 6.32 x 10-8 Ka; = 4.5 x 10-13 For all conjugate acid base pairs: K, XKK where K is for the reaction...
7. (4 points) LiCN is a salt solution. The Ka of HCN is 6.2 x 100, a. Should the salt solution be acidic, basic, or neutral? b. Write the equilibrium reaction for the ion of the salt that contributes to the pH of the solution c. Calculate the pH of a 1.25 M solution of LiCN.
I attempted to answer some of this question, but don't think I'm understanding what's needed. Chem makes my eyes cross... Liquid ammonia, NH3(l), is an ionizing solvent like water. This means that NH3(l) can dissolve many different ionic compounds and can undergo autoionization. Therefore, there can be acidic, neutral, or basic species in solutions of liquid ammonia. (a) (Write the chemical equation, using the Brønsted-Lowry perspective, that describes the autoionization of NH3(l). --NH3 --> NH2 + H- ?? (b) Identify...
11. For each of the following, is the solution acidic, basic, neutral, or cannot be determined? For each, write the equation for the dominant equilibrium which determined the pH, and justify your pH prediction. Kw 1.0 x 1014 a. 100 mL of 0.10 M K HPO4 Ka 7.5 x 103 Ka2 6.2 x 108, and Kas -4.8 x 10-13 for HsPO4 100 mL of 0.10 M LiH2PO4; see Part a for Ka values b. c. 100 mL of 0.10 M...