Chemistry help!? 1. Sketch and fully label a titration curve for 0.09660 M base with a...
please answer and explain everything fully
1. Sketch and fully label a titration curve for 0.09660 M base with a K = 2.4 x 10 titrated with 0.1224 M HNO, Calculate start and end point pH values, the equivalence point volume (why can't you calculate the end-point volume?). There are at least ten points of interest on this curve to grade.
(5) Sketch the titration curve for the titration of 0.1 M HCI with 0.1 M Na0H used as the titrant. Calculate and label the initial pH, equivalence point volume, and equivalence point pH. 3.
Sketch what a titration curve would look like?
1. Consider the titration of 50.00 mL of 0.01550 M NH3 with 0.03720 M HNO3. A. Sketch what a titration curve would look like for this titration, making sure to: Label both axes Illustrate a curve with the appropriate shape Indicate the location of the equivalence point on the curve (you do not need to identify its exact location on the axes) alenrennint in this titration, the titrated solution will have a...
Sketch a pH titration curve if 100.0 mL of 0.125 M NH3 solution is titrated with 0.15M HCl. Note the following three items on the curve. K, for NHa 1.8 x 105 pH= Calculate the starting pH (no HCl added) vol (mL)= Calculate the volume of HCl added to reach the equivalence point pH = Calculate the pH at the equivalence point.
What is the shape of the titration curve (plot of pH vs. mL of added base) for titration of a weak acid by a strong base? In a titration, 10 mL of 0.10 M HF was titrated with 0.20 M KOH. Calculate the pH of the resulting solution after the addition of the following volumes of base: 0 mL, 2.5 mL, 5.0 mL, and 6.0mL. What volume of base is needed to reach the equivalence point? What species is present...
Strong acid-titrated with strong base. Suppose the titration was reversed in question 2. If you titrated 30.0 mL of 0.1 M HCl with 0.1 M NaOH, indicate the approximate pH (a) at the start of the titration and (b) at the equivalence point. (c) What is the total volume of solution at the equivalence point? Add this curve to your sketch in question 2. 3. la. 1.0; b. 7.0; c. 60 mL]
Use the titration curve of a weak acid with a strong base below to answer the following questions. Identify the Equivalence Point of Titration and label it on the titration curve below. (ii) What is the Titrant (iii) From the graph, what is the [H^+] and the volume of NaOH used to reach the equivalence point. (iv) Calculate the [OH^-] at the equivalence point (v) What is the pKa of the acid used for titration? (vi) Calculate the Ka of...
A. Match each type of titration to its pH at the equivalence point. Weak acid, strong base Strong acid, strong base Weak base, strong acid pH less than 7 pH equal to 7 pH greater than 7 B. A 56.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 28.0 mL of KOH. C. Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8 x 10^-5) with 0.20 M HNO3....
Sketch a pH vs. Volume added graph (titration curve) for a diprotic acid being titrated with NaOH. Label the axis and equivalence points.
13. Sketch a titration curve for the titration of a monoprotic weak acid HA with a strong base. The titration reaction (neutralization) is: HA + OH + H2O+ A On the curve, clearly label the points that correspond to: i. the equivalence point ii. the region with maximum buffering iii. pH = pka iv. pH depends only on [HA] v. pH depends only on [A-] vi. pH depends only on amount of strong base added.