Write products of the following acid-base reaction. Label the acid, base, conjugate acid and conjugate base. Indicate which side is favored in an equilibrium.  HPO4 2- + HC6H5O7 2-

The conjugate to a strong acid is a Weak acid Strong acid Negligible acid Weak base Strong base Negligible base and the conjugate to a weak base is a Weak acid Strong acid Negligible acid Weak base Strong base Negligible base

Complete the following Conjugate equation.  NH4+ - H+ ------>

Draw the most likely conjugate base resulting from this acid-base reaction. Include all lone pairs. Ignore inorganic byproducts. NaH H :O: Q

For the following reaction, K < 1. Classify each of the reactants and products based on their strength as Bronsted-Lowry acids or bases. C₂H5NH+ + C₂H₂O4 HC9H7O4 + C5H5N CyH5NH* HC₂H₂O4 C5H5N C₂H₂O4 Clear All Stronger Bronsted- Lowry acid Weaker Bronsted-Lowry acid Stronger Bronsted- Lowry base Weaker Bronsted-Lowry base

If you mix equal amount concentrations of reactants and products, determine which direction the each of the following reaction proceed? Use the table of acid-conjugate strength (NOT Ka) to explain your answer. CH3-(aq) + CH3CO2H (aq)  -> CH3CO2-(aq) + CH4(aq)

The ratio of the hydronium (H3O*) ion concentration to the concentration of acid present at the start of a reaction multiplied by 100 is known as the Base dissociation constant Percent dissociation Acid dissociation constant Equilibrium constant

What is the product of this acid base reaction assuming a 1:1 reaction? H₂N + HCI NH₂

Assign each species on the left to a category on the right. LiOH HCIO C5H₁1N CH3COOH Clear All strong acid weak acid strong base weak base