Predict the products of each reaction, and whether the solution at equilibrium will be acidic, basic, or neutral. 1. P4O10 + 6H2O (l)----> 2. Na2O + H2O(l) ------> 3. N2O5 + 3H2O (l)------>

10. Which side of the equation does the acid-base equilibrium favor? вхь о: `ОН + a : + b ОН

What is the conjugate base in this reaction: H,PO,+ H,O H,O+H,PO, O H.0+ O HO O HPO, O OH

h To add an 0 atom in basic solution, add 2 OH" to the side that needs the O atom, and also add an H20 to the other side. (OH has one more O than HOH). How many H20 molecules should be added to the left side? How many OH ions should be added to the right? H20 + CIO3 - CI" + OH Number of H50 molecules = 1 Number of OH ions =2

When this reaction occurs H₂O + NH3 -> -OH + NH4+ Which of the following statements are correct? OH₂O is the Bronsted Lowry acid OH₂O is the Bronsted Lowry base ONH3 is the Bronsted Lowry acid ONH3 is the Bronsted Lowry base OOH is the conjugate acid OH is the conjugate base NH4 is the conjugate acid O NH4 is the conjugate base

Boron trifluoride, BF3, will react with a fluoride ion to form BF4-. Which species, if any, acts as a Lewis acid in this reaction? BF4- the solvent F- none BF3

Indentify the conjugation acid-base pairs in the following reactions. An acid donates a proton to become a conjugate base. A base accepts a proton to form a conjugate acid.

Q)1

Which of these acids has the lowest pH at equilibrium? Acid Ka HIO3 1.7 x10-1 HCIO2 1.1 x10-2 HCOOH 1.8 x10-4 CH3COOH 1.8 x10-5

Identify the conjugation acid-base pairs in the following reactions. An acid donates a proton to become a conjugate base. A base accepts a proton to form a conjugate base.