The major concept that is used in following answers is how the conjugate base/acid of an acid/ base behaves.
Q. 2a. Ans: Combination of strong acid with strong/weak base has initial value 1 or close to 1.
Q. 2b. Ans: Yeah, these are the expected results. we are measuring the pH of solution in conical flask. So, when we havent added any base to it, the pH of acid is the initial pH.
Q. 3. Ans: pH at equivalence point is neutral for SA (strong acid) + SB (strong base) and WA (weak acid) + WB (weak base), acidic for SA+WB, basic for WA+SB. Yeah, these are the expected results. We can understand it by considering the product formed after reaction of acid and base.
Q. 4. Ans. For SA + SB and WA + SB pH=9 on vertical region.
b) For alll the mentioned cases, time of the indicator color change and time at the equivalence point matches. Actually the color change of an indicator generally termed as end-point and it depends on how precisely the color change is observed. End point can vary depending upon various factor like concentration of indicator etc. Equivalence point can only be obtained when pHmetric machine is used and the above mentioned graphs are plotted.
Q. 7. Ans. For the case of strong acid and strong base indicator changing color at pH 5 or 9 works well. This can be understood by looking into the mentioned plot in the question. Both pH=5 and pH =9 falls into the vertical region of the curve, hence both type of indicator can change color during the sudden jump in pH.
(write clearly please.) the data for the table was found by looking at these 4 graphs:...
Explain and write neatly please
The data for the table was found by looking at these 4
graphs.
Answer 5a&b, 8a&b, and 9 please.
Table 1 - Equivalence Point and Indicator Color Change Time of Indicator Color Time at Equivalence pH at the Change(sec) Point (sec) Equivalence Point 140 140 7.5 165 165 8.6 Initial pH Final pH 11.8 Acid-Base Combination HCI + NaOH HC,H,O + NaOH HCI + NH OH HC,H,O + NH,OH 1 3.9 12 140 140 5.0...
DATA AND CALCULATIONS Time at equivalence point (s) Time of color Trial *Equation for acid-base reaction change (s) NaOH+HCI - 21 0s 1 250.5 NaOH+ HC2H3O2- 2 8l.55 99s 3 NH3+ HCl- 930s 4 NH3 + HC2H3O2- 90.55 81.Os Complete the reactions above. Attach copies of all four graphs to this report. 1. 2. Examine the time data for each of the Trials 1- -4. In which trial(s) did the indicator change color at about the same time as the...
based on thw data can someone solve question number 1, 2, 3,
4
18 Acid-Base Reactions Titration Curve Consider a 10. mL sample of 0.10 M HCI. a) What is the pH of the solution? b)How many ml. of 0.10 M NaOH would be required to neutralize it? c) what is the pH of the neutralized solution? d) What would the pH of the solution be if you added 20. mL of NaOH? volume ofvolumef 0.10 M HCI 0.10 M...
EXP
#9:Pre-Lab
answer question 3, attached below is page two to
reference!
Instructor Name: Student Name: 3. An unknown solution gives the following sequential results for color when indicators are added (shown below). Using the corresponding color ranges from the table on page 2, estimate the approximate pH range of this unknown solution. Explain. Bluish purple Bromphenol blue: Yellow Methyl Red: Blue Bromothymol Blue: Colorless Phenolpthalein: For a titration, pure indicators are used because the goal is to use an...
can
someone help me answer these 5 questions and figire this graph out
please?
Acid-Base Titration of a Weak Acid with a Strong Base: Determination of K. Introduction: You will be titrating a solution of a weak acid with 0.100 M NaOH, while monitoring the reaction using a pH meter. Weak acids have characteristic acid-ionization constants, K. The purpose of this lab is to use the titration to determine the value of this constant for the weak acid called “benzoic...
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u help? im not sure about my answers
Question 6 2 pts A 50.0 mL sample of 0.20 M HCl(aq) is titrated with 0.10 M NaOH(aq) (adding NaOH to HCI). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added base. Assume that the volumes of the solutions are additive. NaOH HCI Parta) [Select ] after 1) After adding 20 mL of the NaOH solution, the...
It's a weak acid strong base titration
Experiment 4: Identification of an unknown acid by titration Page 2 of 15 Background In this experiment, you will use both qualitative and quantitative properties to determine an unknown acid's identity and concentration. To do this analysis, you will perform a titration of your unknown acid sample-specifically a potentiometric titration where you use a pH meter and record pH values during the titration, combined with a visual titration using a color indi- cator...
Which of the following is true for the titration of a weak acid with a strong base? O a. The pH at the equivalence point is acidic. b. A buffer solution is formed before the equivalence point. OC. The initial pH equals -log (conc. of the acid). Od. The indicator changes its color at the half-neutralization point.
3. 0.7253 g sample containing an unknown weak acid HA was dissolved in 50 mL water and titrated against 0.1555 M NaOH, requiring 48.11 mL to of NaOH to reach the end-point. During the titration reaction, the pH of the solution is 3.77 when half of the HA is neutralized and the equivalence-point pH is 8.33. (a) State two ways to standardize the NaOH used in the titration. (b) Suggest and explain an indicator that can be used in the...
What is the approximate pk, for the weak acid. (d) Excess hydroxide ion (c) Equivalence point pH (b) Buffer region ta) Weak acid a) Weak acid 12 14 1 8 10 Volume of NaOH (ml.) Titration curve for the titration of a weak acid with a strong base.