For each of the following aqueous reactions, identify the acid, the base, the conjugate base, and the conjugate acid. a. Al(H2O)63+ + H2O H30+ + Al(H2O)5 (OH)²+ b. H2O + HONH3+ = HONH, H3O+ + с. НОСI + CеHs NH2 OCI C6 H5 NH3+ +

1donsify the apid, base , conjugate acid and conjugate base in The follaing reachon HPOU t AzO > HO t Ag PO 4

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

Which of the following statement best explain why the acidity of carboxylic acids is greater than those of the alcohols? a. Alcohols behave as neutral compounds in aqueous solution. b. Alcohol has the ability to donate proton to becomes a negative ion called an alkoxide ion, RO– c. When a carboxylic acid donates its proton, it becomes a negatively charged ion, RCOO−, called a carboxylate ion which is more stabilized by resonance. d. The OH group in alcohol is less charged and often more difficult to release electron for chemical reactions.

For a certain acid pK = decimal places. pH = 0 4.49. Calculate the pH at which an aqueous solution of this acid would be 2.9% dissociated. Round your answer to 2 X 5

Calculate the pH of each of these solutions.  is the solution acidic, basic, or neutral ?.       a.  a solution with a OH- concentration of 5.5 x 10-12 M       b.  a solution with a H3O+ concentration of 3.2 x 10-8 M       c.  a solution with a pOH of 7.00

Four solutions of an acid dissolved in water are sketched below, as if under a microscope so powerful individual atoms could be seen. The same volume of solution is shown in each sketch. Rank the solutions by the strength of the dissolved acid. That is, select 1 under the solution of the strongest acid, 2 under the solution of the next strongest acid, and so on. =H₂0 Note: Solution 1 (Choose one) Solution 3 (Choose one) Solution 2 (Choose one) Solution 4 (Choose one) X 5

Part 1- What is the conjugate acid of H2PO4−? of NO3−? Part 2 -Write the balanced chemical equation for the neutralization reaction between Sr(OH)2 and H3PO4. What is the salt? Part 3 - If the concentration of H3O+ is 3.5 × 10-3 M, the concentration of OH−− is ________ M. (Show your Calculation) Part 4- Identify each substance as an Arrhenius acid, an Arrhenius base, or neither. b) HNO2 c) Ba(OH)2

In a basic solution at 25°C, O a. [H3O+]> [OH]. O b. OC. [H3O+]> 1.0 x 10-7. O d. [OH-]> 1.0 x 10-7. O e. [H3O+][OH-]> 1.0 × 10-14. [H3O+][OH-]<1.0 × 10-14