Exp 3 Part A pH Titrations Slides

1. The reaction of ??? with ???3 is presented by the unbalanced chemical reaction below: ___ KOH(aq)+ ___ HNO3 (aq) ---> ___ KNO3 (aq)+ ___ H2O(l)Calculate the molar concentration of Nitric acid (???3) when 40.5−?? of 0.674 ? ???is required to quench 101.0?? of Nitric acid over phenolphthalein indicator.

A third titration used 22.5 mL of NaOH solution to neutralize 25.0 mL of 1.013 M HCl.  Determine the molarity of the NaOH solution. Calculate the average Molarity of the NaOH solution, report this to 3 sig figs.

This is about determinition of acid content in vinegar through titration, please answer the questions. Please answer only the items nummber 4-5. i only put other questions for guide. 1. What is the purpose of standardization? 2. What is the primary standard used (name and formula)? ANS: KHP 3. Suppose that the KHP is not completely dry. Will the reported molar concentration of the sodium hydroxide solution be higher, lower, or unaffected? Explain. 4. In preparing the buret for titration the final rinse is with the NaOH titrant rather than with distilled water. Explain. 5. The procedure suggests the addition of only 2 drops of phenolphthalein. What will be the effect to the analysis if larger amount of phenolphthalein is added?

A student prepares a weak acid solution by dissolving 0.2400 g HZ to give 100. mL solution. The titration requires 30.0 mL of 0.1025 M NaOH. Calculate the molar mass of the acid. (a) Would the molar mass be too high, too low, or unaffected if the student accidentally used 0.1400 g in the calculation? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated  (b) Would the molar mass be too high, too low, or unaffected if the student accidentally used 20.0 mL instead of 30.0 mL? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated

To prepare the buffer, a total volume of 500 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.45 M. (Remember the lesson on dilution: C1V1=C2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution?  (Supply answer up to the 2nd decimal point)

Concentration of HCl--0.35M Volume of HCl- 24.35 mL  Volume of NaOH - 36.44 mL   The data above refers to a titration of NaOH with a known concentration of HCl.  Calculate the moles of NaOH at the endpoint.

Label the equivalence point on the graph of pH versus volume of the titration of a strong acid and strong base shown below.  a. What volume of base was needed to neutralize the acid? b. What is the pH at the equivalence point?Titrations and pH CalculationsShow work on all calculations and include c. How does the number of moles of hydronium ions and hydroxide ions compare at theequivalence point?

Please Explain. Thank You Write a plan and theory with equations and pictures  An unknown solid sample is given to you. It is a mixture of KHP & NaCl. Your goal is to find % of KHP in this given unknown sample.  Given: Standardized NaOH (made last week) Unknown KHP Sample Computer with pH probe- Logger Pro-Vernier program Digital Burette pH meter Is KHP an acid or base ?_____________ Is it monoprotic or diprotic ?__________________ What is its formula weight ?_________________________________________ g/mol Is soluble in water?___________________________________________________________

Solve for titer. Pls show me the solution or step by step process so I can follow. Thank you

Given an unknown solid mixture of NaCl and Na2CO3, determine the mass percent of each compound via titration.   I'm given 0.1 M HCl standard solution and bromocresol green pH indicator, as well as standard lab equipment including a buret. What would the procedure for this look like? Will upvote

A student prepared a 1:1 buffer, for which [HAc] = [Ac-] = 0.05182 M. Using their 1:1 buffer and a 0.10229 M HCl solution, the student prepared Solution C in Part 3 of the experimental procedure. Given this information, how many moles of Ac- were there in the student's Solution C after a reaction took place? Report your final answer, in moles, to 6 decimal places and only include the numerical value (no units). Solution C contains 20mL of buffer and 5mL of HCl.

For an acid-base titration, the moles of the acid should be equal the moles of the base. 30 mL of aliquot of a 0.23N HCl is placed in an Erlenmeyer flask and 2 drops of phenolphthalein was added. It was titrated and had an intial reading of 15.8 The normality of the solution is found to be 0.52N. (a) How much of the NaOH solution is used for the titration? (b) What is the final reading on the buret?

Please Explain. Thank You Write a plan and theory with equations and pictures  An unknown solid sample is given to you. It is a mixture of KHP & NaCl. Your goal is to find % of KHP in this given unknown sample.  Given: Standardized NaOH (made last week) Unknown KHP Sample Computer with pH probe- Logger Pro-Vernier program Digital Burette pH meter What volume of a 0.100 M NaOH(aq) is required to neutralize 0.256 g of  KHP ? 0.556 g of an unknown solid sample (KHP+NaCl) requires 12.45 mL of 0.100 M NaOH(aq). Calculate the % of KHP in the unknown solid sample.

in a container with HCl solution with volume 400 ml and pH = 1, add the salt of PbCl2. Calculate how many grams of PbCl2 can be dissolved in this container, when we know that Kpt of PbCl2 = 1.6 × 10-⁵?

To prepare the buffer in the previous problem, a total volume of 500 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.99 M. (Remember the lesson on dilution: M1V1=M2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution?  (Write your answer in 3 decimal places without the unit).   PREVIOUS PROBLEM:

Consider the Heat of Solution Practical that was conducted.   Temperature (oC)   Amount of NaOH ( 0.015M) used to reach end point of titration (ml)     40      42     35      35     30      26     25      23     20      16   Use the data provided above in order to determine the heat of solution. Include any necessary graphs.

a). What are acids, bases and buffers?b) What are the different types of buffers? Describe the mechanism howbuffers resist pH change in a system.c) Elaborate all chemical reactions in the standardization of NaOH withKHP?d) Why do you need to use KHP in the standardization of NaOH?e) Why is phenolphthalein used as an indicator in this experiment?f) Compare and contrast: endpoint vs equivalence point.g) Discuss the role of acids, bases, buffers and pH in water qualitymonitoring and post-harvest fisheries.

Moles SCN- used in titration (mol)Moles of Agt in 20.0 mL titrated (mol) [Ag*lequil (M)X= [Ag*Jinit - [Ag*lequil = Change (M)   solve for flask d e and f

4. About 10 mL of concentrated HCl was transferred to a 1-L bottle and diluted to with water. When this solution was used to titrate a sample of pure sodium carbonate weighing 0.3054 g, it took 35.06 mL to reach the methyl red end point. Calculate the molarity of the HCl solution.