Use the curve shared in contents -> solubility and solutions -----> solubility curve to answer the following questions: a. How much max mass of potassium nitrate does dissolve in 500g of water at 40 degree C? b. What mass of potassium chlorate will come out of 200g of solution if its temp drops from 70- 10 degree? C. At what temp the solubility of sodium chloride and potassium chlortae is same. Explain, how did you get the answer by mentioning the numerical value.

Use the curve shared in contents -> solubility and solutions -----> solubility curve to answer the following questions: a. How much max mass of potassium nitrate does dissolve in 500g of water at 40 degree C? b. What mass of potassium chlorate will come out of 200g of solution if its temp drops from 70- 10 degree? C. At what temp the solubility of sodium chloride and potassium chlortae is same. Explain, how did you get the answer by mentioning the numerical value.

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter18: Acids And Bases

Section: Chapter Questions

Problem 18STP

See similar textbooks

Similar questions

Using the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.
Maleic acid (H2C4H2O4, represented by H2M) is the precursor of malic acid widely used in industry. food as an acidulant and in the pharmaceutical industry it is used in the treatment of wounds. This acid can be determined by neutralization titration. Answer the items below about this determination. Considering a 15.0 mL sample of maleic acid-based product used in industry, determine the maleic acid concentration, in mol/L, in the sample knowing that 21.7 mL of a solution of 0.1120 mol/L NaOH for complete neutralization of this acid. How many grams of maleic acid were in the sample analyzed and what is its percentage (%, m/v) in the sample? [Answer; m=0.1405 mol L-1; percentage = 0.9365%] NaOH(aq) + H2M(aq)  Na2M (aq) + H2O(l) Suggest an appropriate indicator for the titration of this acid by looking at the titration curve profile below (IMAGE)
A 0.1-L unbuffered solution needs the pH adjusted from 6.8 to 2. How many microliters of a 6 molar HCI solution need to be added to adjust the pH? Report your answer to four decimal places. For this question: • Assume the volume of HCI being added is negligible and the total volume of the solution does not change. • The volume of the solution is *not* 1 L like it was in the practice pools. • The question requests your answer be reported in uL (microliters)!
A biology experiment requires the use of a nutrient fluid buffered at a pH of 4.85, and 659 mL of the solution is needed. It has to be buffered to be able to hold the pH to within =0.10 pH units of 4.85 even if 5.00 x 10 mol of OH or 5.00 x 10 mol of H* ion enter. Record all your answers to three (3) significant figures. Pick the best acid and its sodium salt that could be used to prepare the solution. O Hydrocyanic acid and sodium cyanide (pK, = 9.21). O Nitrous acid and sodium nitrite (pk, = 3.15). Acetic acid and sodium acetate (pK, = 4.74). O Hydrofluoric acid and sodium fluoride (pK, = 3.17). Hint Calculate the minimum number of grams of the acid and its sodium salt that are needed to prepare the buffer solution. Mass acid i Mass sodium salt = i Hint Calculate the molar concentration of the acid and its sodium salt that are needed to prepare the buffer solution. Concentration acid = M Concentration sodium salt = M Hint on
The hydronium ion concentration of an aqueous solution of 0.558 M isoquinoline (a weak base with the formula CoH-N) is ... M. = LO°H]
Aspirin (acetylsalicylic acid) is absorbed from the stomach in the free (non-ionized) acid form. If a patient takes an antacid that adjusts the pH of the stomach contents to 2.59 and then takes two 5-grain aspirin tablets (total 0.65 g), how many grams of aspirin are available for immediate absorption from the stomach, assuming immediate dissolution> Also assume that aspirin does not change the pH of the stomach contents. The pKa of aspirin is 3.5, and its formula weight is 180.2.
Aspirin (acetylsalicylic acid) is absorbed from the stomach in the free (non-ionized) acid form. If a patient takes an antacid that adjusts the pH of the stomach contents to 2.59 and then takes two 5-grain aspirin tablets (total 0.65 g), how many grams of aspirin are available for immediate absorption from the stomach, assuming immediate dissolution> Also assume that aspirin does not change the pH of the stomach contents. The pKa of aspirin is 3.5, and its formula weight is 180.2. _______ mg
A 0.1-L unbuffered solution needs the pH adjusted from 3.5 to 2. How many microliters of a 12 molar HCl solution need to be added to adjust the pH? Report your answer to four decimal places. For this question: • Assume the volume of HCI being added is negligible and the total volume of the solution does not change. • The volume of the solution is *not* 1L like it was in the practice pools. • The question requests your answer be reported in pL (microliters)!! Name: Duration: CalculatingChangelnpH (04:33) 04:33 15 Jan 2018 04:04 PM Added: Watch Media
Consider an analyte solution of 50.0mL of 0.050M hydrochloric acid, HCl, titrated against 0.10 M sodium hydroxide, NaOH (the titration you will be performing in the lab!). (g) After adding 37.50mL of the NaOH, 50% past the equivalence point, what ions or molecules are present in the solution? (h) Which of the species you identified in part (g) will determine the pH of the solution?
Definition/explanation of titer in chemistry.
What is an acid–base indicator? Define the equivalence(stoichiometric) point and the end point of a titration.Why should you choose an indicator so that the twopoints coincide? Do the pH values of the two pointshave to be within 60.01 pH unit of each other?Explain.
This question is about acid base titration: Osama a student, performed an acid base titration involving a standard solution of Sodium hydroxide (NaOH) (RMM = 40) against unknown HCl solution and obtained the following results. Mass of Sodium hydroxide (NaOH) dissolved in 250 ml volumetric flask = 3.6 g 2.Volume of Sodium hydroxide used in the titration = 23 ml 3.The mean volume of HCl titrated with 25 ml Sodium…

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Matter and Change

Chemistry

ISBN:

9780078746376

Author:

Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:

Glencoe/McGraw-Hill School Pub Co

General, Organic, and Biological Chemistry

Chemistry

ISBN:

9781285853918

Author:

H. Stephen Stoker

Publisher:

Cengage Learning

Living By Chemistry: First Edition Textbook

Chemistry

ISBN:

9781559539418

Author:

Angelica Stacy

Publisher:

MAC HIGHER

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Introductory Chemistry For Today

Chemistry

ISBN:

9781285644561

Author:

Seager

Publisher:

Cengage

Chemistry: Matter and Change

Chemistry

ISBN:

9780078746376

Author:

Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:

Glencoe/McGraw-Hill School Pub Co

General, Organic, and Biological Chemistry

Chemistry

ISBN:

9781285853918

Author:

H. Stephen Stoker

Publisher:

Cengage Learning

Living By Chemistry: First Edition Textbook

Chemistry

ISBN:

9781559539418

Author:

Angelica Stacy

Publisher:

MAC HIGHER

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Introductory Chemistry For Today

Chemistry

ISBN:

9781285644561

Author:

Seager

Publisher:

Cengage

SEE MORE TEXTBOOKS