Use the Acid-Base Table to write net equations and determine the equilibrium constants for the Bronsted acid-base reactions that occur when aqueous solutions of the following are mixed.
Substances | Acid(1) + Base(2) -> Base(1) + Acid(2) | K |
---|---|---|
HC2H3O2 + Na2HPO4 | ||
KNO2 + HIO3 |
||
HF + KClO |
Use the Acid-Base Table to write net equations and determine the equilibrium constants for the Bronsted...
Use the Acid-Base Table to write net equations and to determine the equilibrium constants for the Bronsted acid-base reactions that occur when aqueous solutions of the following are mixed. See the instructions for writing chemical equations given above. Reactants Acid(1) + Base(2) = Base(1) + Acid(2) K a) HClO4 and KF b) HIO3 and NH3 c) HCN + KClO Click here to preview your answer.
Write net Bronsted equations and determine the equilibrium constants for the acid-base reactions that occur when aqueous solutions of the following are mixed.Instructions:Enter all substances in the order listed at the top of the column.Use a carot to indicate a superscript, but do nothing for subscripts.Use a hyphen + greater than (->) for yields.Click on the eye symbol to check your formatting.Report K to three sig figs even though it is good to only two.Group 1A and 7A ions (except...
Write the net equations and determine the equilibrium constants for the acid-base reactions that occur when aqueous solutions of the following are mixed. (Use the lowest possible coefficients. Omit states-of-matter in your answer. Your reaction arrow may be either a right arrow (-->) or an equilibrium arrow (<=>), depending upon the value of Keq for the reaction. Use the Acid/Base Table. (a) acetic acid (CH3COOH) and ammonia, K= (b) hydrochloric acid and sodium hydroxide (Please write the conjugate acid and...
Write the net equations for the acid-base reactions that occur when aqueous solutions of the following are mixed. (Use the lowest possible coefficients. Omit states-of-matter in your answer. Your reaction arrow may be either a right arrow (-->) or an equilibrium arrow (<=>), depending upon the value of Keq for the reaction. Do not forget about spectator ions. (a) acetic acid (CH3COOH) and ammonia (b) hydrochloric acid and sodium hydroxide (Please write the conjugate acid and base separately.) (c) KHSO4...
Write correct balanced molecular, total ionic, and net ionic equations for the reactions that occur when the following substances are mixed. All are in aqueous solution except as noted. 1) magnesium chloride and sodium carbonate 2) aqueous ammonia and acetic acid
1 a) Write the aqueous acid dissociation reactions for an acid and base dissociation reaction for a base according to the Bronsted-Lowry definition b) Determine conjugate bases of acids and acids of bases c) Write the equilibrium expression for an acid or a base aqueous dissociation d) Evaluate strength of an acid or base based on its Ka or Kb or pKa or pKb. e) Apply Kw at 25oC and at different temperatures. f) Solve for the pH of strong...
1) write molecular, complete ionic, and net ionic equations for the reactions that occur, if any, when solutions of the following substances are mixed: a) nitric acid and barium carbonate, b) zinc chloride and lead nitrate, c) acetic acid and sodium hydroxide, d) calcium nitrate and sodium carbonate, e) ammonium chloride and potassium hydroxide.
whats the answers 1. Write molecular, complete ionic, and net jonic equations for the reactions that ove if any, when solutions of the following substances are mixed: (a) ammonium bromide and silver nitrate (b) potassium phosphate and ferric chloride (c) sodium sulfide and cadmium nitrate (d) ammonium sulfate and sodium hydroxide QUESTIONS: 1. Write molecular, complete ionic, and net ionic equations for the reactions that occur, if any, when solutions of the following substances are mixed: (a) ammonium bromide and...
2) Predicting acid-base equilibrium. Write equations for the following acid-base reactions and predict (by trends) which side the equilibrium prefers: a. CH3CH2OH + NaN(CH3)2 b. CH3NH3 + + CH3O c. CH3CHFCO2H + FCH2CH2CO2 - d. NaOH + H2S e. CF3CO2H + CH3CO2
#2 & 3 Identify the following species in water, as Bronsted Acids [A] or Bronsted Bases [B]: H_3O^+; H_2SO_4; OH^-; HCN; CH_3COOH; CH_3NH_2 WRITE NET Ionic Equations for the reactions of H_2PO_4^-, an amphiprotic ion, with aqueous solutions of HCl KOH Give the conjugate base for each of the following acids: HI HSO_4^- H_2CO_3 C_2H_5NH_3^+ Give the conjugate acid for each of the following bases: NH_3 O^2- H_2O PO_4^3- Identify the conjugate acid-base pairs in each of the following reactions:...