1st question
end point | equivalence point |
Point where the indicator changes colour | The point at which the titrant is chemically equivalent to the analyte in the sample |
Comes after the equivalence point | Comes before the endpoint |
2nd question
both the molar mass and Pka values will be wrong
this can be explained as follows
1) if the concentration of HCl is wrong we will end up getting wrong end point value which will lead to wrong molar mass of the unknown
2)since the concentration itself is wrong concentration of H+ ion will also be wrong hence pH and Pka will also be wrong
This is chemistry lab, Analysis of Unknown Base sample :Using Titation Curve to Deterime formula ...
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...
grams of KHP 0.6413 mL NaOH needed to titrate KhP to endpoint 38.80 Grams of unknown acid: 1.5106 mL NaOH needed to titrate unknown acid to endpoint 33.55 need to know molarity of NaOH solution and Molar mass of unknown acid. Please help and show work! CHEM 265 LAB EXPERIMENT NUMBER 4 DETERMINATION OF THE MW OF AN UNKNOWN ACID This experiment utilizes a titration to determine the molecular weight of an unknown acid. In this experiment, the endpoint of...
please answer all the parts Supplemental Questions - Titration Lab, 1. Indicate how each of the following would affect the values of K, for the weak acid unknown and for the dibasic salt and the value of the molar mass for the dibasic salt (Would the determined values be higher or lower than the actual values?). Use larger, smaller or no change. And as always....Explain. a. The titrant (either the NaOH or the HCI) molarity is actually HIGHER than that...
A thorough explanation would sure be appreciated!!!! Thank you!! Acid-Base Chemistry: Unknown Acid Analysis (in two experiments) Introduction In this experiment you will titrate a monoprotic weak acid with a strong ak acid with a strong base in the nd using a pH meter (Exp 2). An analysis of concentration and molar mass of the the titration data will allow you to determine the concentration and more unknown acid (Exp 1) and the ionization constant Ka (Exp 2). At the...
1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCl stock solution. In your response to this question, be very specific about the quantities of stock solution and deionized water to be used in the dilution and the...
please help with my pre lab additional information Pre-Lab Questions: 1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCI stock solution. In your response to this question, be very specific about the quantities of stock solution and...
Post-lab Questions 1. Ca n you titrate a solution of unknown concentration with another solution of unknown concentrat and still get a meaningful answer? Explain your answer in a few sentences 2. Explain the difference between an end point and equivalence point in a titration. 3. What is the pKa of phenolphthalein? Why is it acceptable to use an indicator whose pKa is not exactly the pH at the equivalence point? 4. What was the concentration of the NaOH solution...
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...
PRE LAB : Volumetric Titrations. (Acid-Base Titrations) Name: ID Date 1. How many mL of a 0.103M NaOH solution are required to neutralize 10.00mL of a 0.198M HCI solution? 2. what is the difference between end point and equivalence point? 3. A titration is performed and 20.70 mL of 0.500M KOH is required to reach the end point when titrated against 15.00 mL of H2SO4 of unknown concentration. Write the chemical equation and solve for the molarity of the acid....
Argentometric Determination of Chloride Using Mohr's Method Experiment 25ml of a solution of AgCl (with an unknown concentration) was placed into a 250ml flask. 25ml of distilled water was then added to the flask followed by a few drops of potassium chromate indicator. This solution was then titrated with 0.1012M AgNO3. It was found that 13ml of AgNO3 was needed to be titrated to the solution to reach the reddish/brown endpoint. V of AgNO3 = 13.00ml, [AgNO3] = 0.1012M, V...