Consider only the first dissociation constant of a 10-4 M solution of boric acid (H3BO3): a) develop the appropriate ionization fraction equations, b) draw a species distribution plot for H3BO3, c) develop the appropriate equations for the buffer capacity of H3BO3,

For each combination of acid and base below, what is the relative pH at the equivalence point of the titration? 1) HCO₂H + NaOH: [Select] CIRC 2) HNO₂ + NH3: [Select] 3) H₂SO4 + LIOH: [Select] 4) HBr + KOH: [Select] <

Find the pH of the equivalence point(s) and the volume(mL) of 0.0588 M KOH needed to reach it in titrations of(a) 23.4 mL of 0.0390 M HNO₂(b) 17.3 mL of 0.130 M H₂CO₃(two equivalence points

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CH3COOH + NaOH → CH3COONa + H₂O If at the beginning you have 1 mol of acetic acid and you have added phenolphthalein as an indicator, when will the end point of the titration be reached? a) When 1 mol of NaOH has reacted b) When the solution changes from clear to a pink color c) When a buffer is formed d) When the solution changes pH

For each scenario below, select the color of the solution using the indicator thymol blue during the titration. When you first add indicator to your Na2CO3 solution, the solution is basic (pH ~10), and the color is [Select] At the equivalence point for the titration, the moles of added HCI are equal to the moles of Na2CO3. One drop (or less!) past this is called the endpoint. The added HCI begins to titrate the thymol blue indicator itself. At the endpoint, the indicator color is [Select] When you weren't paying attention and added too much HCI (~12 mL extra), the color is [Select] When you really weren't paying attention and reached the second equivalence point of Na2CO3, the color is ✓ [Select] blue yellow red orange green Question 9

A buffer solution is prepared which is 0.140 M both in lactic acid (CH3CHOHCO₂H) and in sodium lactate (CH3CHOHCO₂Na). 1.38×10-4 for lactic acid. Ka What is the pH of this solution? = 3.860 You are correct. Your receipt no. is 153-562 When 1.94 mL of 0.120 M HCI is added to 11.0 mL of this buffer solution, what is resulting change in pH? 0.11 Previous Tries Submit Answer Incorrect. Tries 33/99 Previous Tries This discussion is closed.

Determine the pH during the titration of 32.5 mL of 0.333 M ethylamine 4.3x10-4) by 0.333 M HCIO4 at the following points. (C₂H5NH2, Kb (a) Before the addition of any HCIO4 (b) After the addition of 13.5 mL of HCIO4 (c) At the titration midpoint (d) At the equivalence point (e) After adding 49.1 mL of HCIO4 =

Read sec. 14.7 2, then calculate the volume at equivalence and the pH at each of the following volumes of titrant for the titration of a 75.00 mL of a 0.049 mol L1 solution of nitrous acid (pKa = 3.37) titrated with 0.198 mol L' sodium hydroxide. %3D Ve = 18.6 mL VOH pH VOH 7.05 pH : VOH = = 12.1 pH %3D VOH = Ve %3D pH %3D Von = 27.8 pH = VoH = 55.7 pH Submit Question Jump to Answer

25.0 ml of 0.100M NaOH is titrated with HC2H3O2  and 50.0mL of the acid is used to reach the endpoint.          e)Would the compound formed at the equivalence point be acidic, basic or neutral?  Write a hydrolysis equation for the salt formed in a) to support your answer. f) Which indicator should be used for this titration?  g)Sketch a titration curve for this reaction. Label the x and y axes.