Of the following species, HNO2 , PO43- , HCO3- , one is amphiprotic in their reactions with water: Write the two equations needed to represent this fact 2. In the reaction below, Encirle the Lewis base. SnCl4 + 2 Cl- → [SnCl6]^-2

The chemical formulae of some acids are listed in the first column of the table below, and in the second column it says whether each acid is strong or weak. Complete the table. List the chemical formula of each species present at concentrations greater than about 10-6 mol/L when about a tenth of a mole of the acid is dissolved in a liter of water. acid HNO₂ H₂SO3 HBrO3 H Br strong or weak? weak weak strong strong species present at 10-6 mol/L or greater when dissolved in water 10 0 0 0 Ś

Calculate the pH of a 0.22 M solution of hydrazine (NH 2 NH 2 ) given that the base-dissociation constant (Kb) is 1.3 * 10 ^ - 6 . Please provide answer to 4 SF. NH 2 NH 2 (aq)+H 2 O(l) - NH 2 NH 3 ^ + (aq)+OH^ - (aq)

1. Determine whether the following solutions are Bronsted-Lowry acids or bases. Then, write out the chemical equation for the dissociated solution. Additionally, determine the conjugate acid/ conjugate base of each dissociated ion. Solution: Acid/base: Chemical equation: Conjugate Acid Conjugate base: а) HBr (aq) HBr (aq) + H2O (1) = b) OH (aq) ОН (аq) + Н2О (1) c) NH4* (aq) NH4* (aq) + H2O (1) =

What is the most important part of the Bronsted-Lowry theory that is not in the Arrhenius theory of acids and bases? acids create H30* in aqueous solution bases create OH in aqueous solution O acids donate H* to water, bases accept H* from water strong acids have complete dissociation, weak acids have equilibrium dissociation ions can act as weak acids or bases

The chemical formulae of some acids are listed in the first column of the table below, and in the second column it says whether each acid is strong or weak. Complete the table. List the chemical formula of each species present at concentrations greater than about 10 mol/L when about a tenth of a mole of the acid is dissolved in a liter of water. acid HE H₂SO, HI INO, strong or weak? weak weak strong species present at 10 mol/L or greater when dissolved in water 0 0 0 0 X 0.0 $ F &

At room temperature (25°C), 45 mL of a 0.002 M acid solution is fully neutralized by30 mL of a NaOH (aq) solution (pH = 11.95). Determine (through calculations)whether the acid is phosphoric acid (H3 PO4 ), acetic acid (CH 3 COOH), or carbonicacid (H 2 CO3 )

Preparing a strong base solution with a given pH A chemist must prepare 600.0 mL of sodium hydroxide solution with a pH of 13.60 at 25 °C. He will do this in three steps: • Fill a 600.0 mL volumetric flask about halfway with distilled water. • Weigh out a small amount of solid sodium hydroxide and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the mass of sodium hydroxide that the chemist must weigh out in the second step. Round your answer to 2 significant digits. g ☐ x10 ☑ 1/5

Determine the acid,base, conjugate base and conjugate acid in the following reaction: CH3COOH + CO32- --> CH3COO- + HCO3-