a) In a NaOH and HCl titration lab: Suppose you add 40 ml of water instead of the 45 mL. How will this affect the calculations for the molarity of the HCI? (In this case, themolarity of HCl turned out to be 0.559 mol/L). While being specific. Explain why it will not matter or it will make the molarity high or it will make the molarity low.b) if you disregard the instructions to titrate until a persistent blue endpoint is reached and instead conclude the titration at the initial appearance of blue, describe theimpact on the reported molarity of the CoC12 solution. Provide specific details and specify whether the reported molarity will be higher, lower, or remain unaffected.

1]Molarity=Molarity (M) is a measure of the concentration of a solute in a solution. It is defined…

In a NaOH and HCl titration lab: Suppose you add 40 ml of water instead of the 45 mL. How will this affect the calculations for the molarity of the HCI? (In this case, the olarity of HCI turned out to be 0.559 mol/L). While being specific. Explain why it will not matter or it will make the molarity high or it will make the molarity low. If you disregard the instructions to titrate until a persistent blue endpoint is reached and instead conclude the titration at the initial appearance of blue. describe the mpact on the reported molarity of the CoCl2 solution Provide specific details and specify whether the reported molarity will be higher, lower, or remain unaffected.

In a NaOH and HCl titration lab: Suppose you add 40 ml of water instead of the 45 mL. How will this affect the calculations for the molarity of the HCI? (In this case, the olarity of HCI turned out to be 0.559 mol/L). While being specific. Explain why it will not matter or it will make the molarity high or it will make the molarity low. If you disregard the instructions to titrate until a persistent blue endpoint is reached and instead conclude the titration at the initial appearance of blue. describe the mpact on the reported molarity of the CoCl2 solution Provide specific details and specify whether the reported molarity will be higher, lower, or remain unaffected.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

In which of these solutions will HNO2 ionize less than it does in pure water?a. 0.10 M NaClb. 0.10 M KNO3c. 0.10 M NaOHd. 0.10 M NaNO2
A student performs the titration of 88.0 mL of 1.1 M HCI (in flask) with 13.0 mL of 0.20 M NaOH (in burette). What is the pH at this point in the titration? (Hint: Use a barf table.) Your Answer: Answer
Now your turn! Sketch the neutralisation curve when 40 cm³ of 0.50 moldm³ sodium hydroxide solution is added to 20.0 cm³ of 0.40 moldm³ propanoic acid (pKa = 4.9). ● Extension: Consider whether methyl orange is an appropriate indicator to find the end point of this titration MacBook Air
Part 1. With the given information determine the effect of adding acid to the listed solutions in the blank table
Please give answer of the question-F accurate and exact with detailed and complete reasons it must be detailed solution please. I'll rate. Thanks (Only last part-F) detailed solution please
Exactly 100mL of 0.1M HF is titrated with 40 mL of 0.1M calcium hydroxide solution. Calculate the pH of this solution after the titration. HF Ka = 1.6 x 10-5 You must type the answer in the text box below. (You must show all your work on paper to get credit) Edit Format Table
2)Make a rough plot of pH versus milliliters of acid added for the titration of 50.0 mL of 1.0 M NaOH with 1.0 M HCl. Indicate the pH at the following points and tell how many milliliters of acid are required to reach the equivalence point. a)Before the titration starts b)At the equivalence point c)After an additional 10.0 mL of HCL is added after the equivalence point (i.e. equivalence point volume + 10.0 mL)
Interpret pH titration plots. Answer the following about the titration plot shown below, involving a monoprotic acid and base. 20 mL of 0.1M titrand titrated with 0.1M titrant. Data points at 1 mL increments. 14.0 12.0 10.0 5 8.0 6.0 4.0 2.0 0.0 seededood 0 0.0 10.0 مهمه 20.0 30.0 Volume of titrant (mL) (a) Is the species being titrated an acid or a base? (b) Is the species being titrated strong or weak? (c) What is the value of Ka (if a weak acid) or K, (if a weak base) for the species being titrated? If the species is strong (100% dissociated), enter 999. rààààààààà 40.0 50.0
Can you show me how to do this type of question please?
2. Fill in the following table to show the theoretical results for the titration of 1.0 L of 0.20 M acetic acid by adding the designated amount of solid (no volume change) potassium hydroxide, KOH. Show sample calculation of your work. Amount of NaOH added 0.0 mol 0.010 mol 0.020 mol 0.030 mol 0.040 mol Amount of acetic acid remaining pH [H+]
When pH titrations occur, more data points become necessary at the vertical deflection near the equivalence point which is accomplished by adding smaller volumes of base from the pipers before taking the pH of the solution. Why are more points needed at this point in the titration curve? Why can larger volumes be used in the area outside of this region?
A 150 mL solution of NaOH is titrated with HI. Phenol red is the indicator, which is red at high pH values and yellow at low pH values. The indicator be [ Select ] when you first put it into your analyte, before any titrant is added. The indicator will be [ Select] at the endpoint. The indicator will be [Select] V if you overshoot the endpoint and add too much acid.