31) The F- ion can react with BF3, forming the BF4 anion. In this reaction, A) the F-ion is a Brønsted-Lowry base, accepting a proton from the BF3 molecule. B) the F-ion is a Brønsted-Lowry acid, donating a proton to the BF3 molecule. C) the BF3 molecule acts as a Lewis base, donating an electron pair to the F- ion to form a coordinate covalent bond. D) the BF3 molecule acts as a Lewis acid, accepting an electron pair from the F-ion to form a coordinate covalent bond. E) the F-ion is a Lewis base, donating a proton to the BF3 molecule.

Chapter #9, Question #5: The principal anion and cation of Lake Huron, one of the Great Lakes in North America, are, respectively, hydrogen carbonate and calcium.  The concentration of the former is approximately 1.05 mmol L-1.  Calculate the mass of solid calcium carbonate that would remain if 250 mL of Lake Huron water is evaporated to dryness.

18.998 20.180 17 18 CI Ar Chlorine Argon 35.453 39.948 Which of the elements shown will form ions, what will be the charges of those ions, and why will they have those charges?

Write the balanced equation for the neutralization reaction between H, SO, and KOH in aqueous solution. Phases are optional. neutralization reaction:

Calculate the pH for a 0.200 M KClO2 aqueous solution. (Ka for HClO2 is 1.1× × 10–2).

Write the balanced equation for each reaction. Phases are optional. The carbonate ion (CO) acts as a Brønsted base with water. equation: The carbon-containing product from the first reaction acts as a Brønsted base with water. equation: The carbon-containing product from the second reaction decomposes into carbon dioxide gas and water. equation: Consider the products of the reactions. When the carbonate ion reacts with water, is the resulting solution acidic or basic? basic acidic

In this reaction, the Ni2+ functions as a ? Ni2+ +6 NH3 → [Ni(NH3)6]2+ BrØnsted acid Lewis acid Lewis base BrØnsted base

How many moles of water will form if 7.0 moles of NH3 is burned?

List the following acids in order of increasing acid strength: HOCl, HClO 3, HClO 4.     HOCl < HClO4 < HClO3     HOCl < HClO3 < HClO4     HClO4 < HClO3 < HOCl     HClO3 < HClO4 < HOCl     HClO3 < HClO < HClO4

Calculate the concentration of H3O* in a solution of H2SO4 that has a pH of 3.5.