Chem 106 Identification of an Acid Lab Report

Some chemical compounds are listed in the first column of the table below. Each compound is soluble in water. Imagine that a few tenths of a mole of each compound is dissolved in a liter of water. The important chemical speci written in the second column of the table. Use the checkboxes to classify each compound. type of compound (check all that apply) important species present when dissolved in water lonic molecular strong weak strong weak base compound acid acid base C,H,NH, c,H,NH, OH , C,H,NH,, H,0 HC,H,0, H,0", C,H,0,, HC,H,0,, H,0 КОН к", он , н,о H BrO4 H,0", Bro,, H,0

Consider the following chemical equilibrium: HCOO- (aq) + H2O(aq) = HCOOH (aq) + OH- (aq). Which of the following graphs represents the perturbation on the system and the change of pH when HCI is added to the container? III PH PH ↑ time time IV PH Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b || C III d IV pH time time Open Your answer

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Recognizing common acids and bases Some soluble compounds are listed in the table below. Complete the table by filling in the name or chemical formula of each compound, whichever is missing. (If there is more than one way to name the compound, choose the name used when the compound is dissolved in water.) Also classify the compound using the checkboxes. compound NaI 0 12 sulfuric acid HCH₂ CO₂ ammonia name type of compound (check all that apply) strong weak strong weak acid acid base base ionic molecular O O O O O O × 3/5 00 S

A solution is prepared that is initially 0.42M in hydrofluoric acid (HF) and 0.28M in potassium fluoride (KF). Complete the reaction table below, so that you could use it to calculate the pH of this solution. [H,0°]. Use x to stand for the unknown change in You can leave out the M symbol for molarity. [HF] [F] [1,0'] initial change final

Using the table of the weak base below, you have chosen Ammonia as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.65 M in this salt. The desired pH of the buffer should be equal to 8.8. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula 1.8 × 10-5 4.38 x 10-4 5.6 x 10-4 3.8 × 10-10 1.7 x 10-9 Ammonia Methylamine Ethylamine Aniline NH3 CH;NH2 C¿H5NH2 CH§NH2 C;H;N NH,+ CH;NH3+ CH§NH;* CH;NH;* Pyridine C:HNH+ To prepare the buffer, a total volume of 300 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.85 M. (Remember the lesson on dilution: C1V1=C2V2) 4/4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (round off final answer to 3 decimal places)

What will happen if you add a small amount of KOH to a solution containing acetic acid and potassium acetate? The concentration of acetate ion will increase and the concentration of acetic acid will decrease. O The concentration of acetate ion will decrease and the concentration of acetic acid will increase. O The concentration of hydronium ions will increase significantly. O The concentration of hydroxide ions will increase significantly.. pH will drop significantly pH will increase significantly

Using the table of the weak base below, you have chosen Ammonia as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.65 M in this salt. The desired pH of the buffer should be equal to 8.8.

A solution of hydrochloric acid is mixed with an equal volume solution of barium hydroxide. When pH paper is inserted into the resulting solution, the pH was determined to be 7.0. If the initial concentration of the hydrochloric acid solution was 0.5 M, what is the concentration of the barium hydroxide solution?

Drill-type Questions 1. The ionization constant (Ka) of aniline (CSHSNH2) is 2.35 x 10 If 7.285 grams of aniline is dissolved in 100.0 mL of water, what are the equilibrium concentration of all species present? 2. A certain acidic vitamin is essential for all mammals since it plays a role in DNA repair and cell signaling. A 0.439 M solution of this acid is found to have a unknown acid? pH of 2.607. Based on the tabie below, what most likely is the identity of this

In the laboratory, a general chemistry student measured the pH of a 0.580 M aqueous solution of aniline, C6H5 NH2 to be 9.332. Use the information she obtained to determine the K for this base. K(experiment)

Determine the pH of a solution of aspirin (acetylsalicylic acid, HC9H7O4) by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. Initial (M) Change (M) Equilibrium (M) -X NEXT > 652 mg of aspirin (HC9H7O4) is dissolved in an aqueous solution of 237 mL aqueous solution. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. 15.3-x PO annotated-Acid-B....pdf A 0 1 HC9H7O4(aq) + 2.75 x 10-³+x 0.0153 + x 2.75 x 10-3 2.75 x 10-x 0.0153-x 2 H₂O(1) 3.62 x 10-3 3.62 x 10³+x 1.53 x 10-5 3.62 x 10-x 3 H3O+ (aq) + C9H7O4 (aq) 15.3 1.53 x 105+x 0.0153 1.53 x 10-5-x RESET 15.3 + x