HCI flushed 20 milliliters of hydrochloric acid (7 concentration of 0.1 normal, with sodium hydroxide concentration of 0.05 normal, the values of the change in the pH function were: A- before scaling, B- after adding 8 milliliters of , C- at equivalence point, D- after adding 1 milliliters of equivalence point

HCI flushed 20 milliliters of hydrochloric acid (7 concentration of 0.1 normal, with sodium hydroxide concentration of 0.05 normal, the values of the change in the pH function were: A- before scaling, B- after adding 8 milliliters of , C- at equivalence point, D- after adding 1 milliliters of equivalence point

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.22QAP

See similar textbooks

Similar questions

2. Calculate titre of potassium dichromate, in case when 500 ml of the solution contains 1,2230 g of pure salt (М=294,185 g/mol). Express numerical result with an accuracy of: Х,ХХХ.10-х
Prepared buffer solution GivenAmmonia Volume = 68 mL | Ammonia Concentration = 0.17 MAmmonium Chloride Volume = 42 mL | Ammonium Chloride Concentration = 0.13 MDissociation Constant of Ammonia: 1.8x10-5What is the total vol. of buffer
If you were to overshoot tje endpoint in the titration of your unknown acid, would youncalculated molar mass be higher, lower or equal to the actual molar mass
This is the reaction with Acid-Base indicator. Please explain clearly what the result below means. INDICATORS COLOR BLUE LITMUS PAPER TURNS RED RED LITMUS PAPER REMAINS RED CONGO RED RED/PINK PHENOLPHTHALEIN NO CHANGE
Calculate the volume in milliliters of .357 M KOH necessary to titrate .0282 moles of acetic acid to a phenolphthalein end-point. Report the answer with precision of two decimal places. I do not know how to set this up if you could explain how that would be great.
An acid-base indicator is usually a weak acid with a characteristic color in the protonated and deprotonated forms. Because bromocresol green is an acid, it is convenient to represent its rather complex formula as HBCG. HBCG ionizes in water according to the following equation: HBCG + H2O ⇌ BCG- + H3O+ (yellow) (blue) a. Write the Ka expression for bromocresol green based on the equation above. b. When [BCG-] = [HBCG], then show that the expression simplifies to Ka = [H3O+]. If you know the pH of the solution, then the [H3O+] and Ka can be determined. c. What would be the color of the solution if there were equal concentrations of HBCG and BCG-?
How to write the methodology? I have a practical of the MEASUREMENT USING PH METER, I don't know how to write the methodology. Here is the introduction: A pH meter is an electronic device mainly used for qualitative measurement, for thedetermination of acid and the basic value of a solution. Generally, it measures thehydrogen ion concentration/activity [H+] in a solution. It is denoted as:pH = - log10 [H+]In a pure water solution, the concentration of [H+] and [OH-] ions, respectively, rangefrom 1.0 x 10-1 M to 1.0 x 10-14 M. When [H+] is equal to [OH-] as when pure waterdissociates, the hydrogen ion concentration of pure water is equal to 1.0 x 10-7 M orpH = 7.00, defined as a neutral solution at 25°C, to be of temperaturedependent/endothermic dissociation.[H+] = [OH-] = 1.0 x 10-7 MWhen an ionic or polar substance is dissolved in water, it may change the relativenumbers of H+ and OH-. The higher the pH number, the lower the hydrogen ion concentration, and vice versa. Solution with an…
How would the calculated molarity of the HCl solution would be affected (too large, too small,no effect) if bubbles of air were trapped in the Burette tip?
Each indicator gradually changes colour over a range of about how many pH units?
Suppose a change (an error, if you like) was made in the procedure of the experiment. We would to know qualitatively, (higher than the correct value, lower than the correct value, or no change) how this change would affect the calculated hydroxide ion concentration. A suggested method for determining and explaining the answer was given in experiment 7 and is repeated here for one such change, with only the final conclusion missing. Fill it in. For the second change, you do the whole analysis. Change 1 – The endpoint was overshot (too much titrant was added). Quantity Measured value (what actually happened) “True” value (what should have happened) (Compared to true value) measured value is Why? Initial burette reading Correct Beginning of titration was ok. Final burette reading 31 mL, say 30 mL, say Too high VNaOH Too high so change in the same direction. Correct Pipetting was ok. Correct Too _________ The numerator is correct; the denominator too high. Change 2 –…
A 4.0520g sample of HCl, specific Gravity 11.18, required 44.15ml of 0.9035M of Sodium Hydroxide in titration, compute for percent purity. Please explain thoroughly. Final answer in percent.
Calculate the volume in milliliters of 0.368 M KOH necessary to titrate 0.0209 moles of acetic acid (HOAc, HC2H3O2) to a phenolphthalein end-point. Report the answer with a precision of two decimal places.