1. Potassium hydroxide (KOH) is a strong base in aqueous solution. Give the pH of a KOH solution with a concentration co = 4.0 x 10-3 mol.L-1. 2. A hydrochloric acid (HCI) solution of 0.15 M concentration and volume V = 120 mL is available. 35 mL of this solution is taken and added to 100 mL of water. Calculate the concentration of all the species in solution and the pH of the new solution. 3. 100 mL of an aqueous solution of KOH at 0.01 mol.L-1 has been prepared. Give the pH of the solution. To this solution is added 50 mL of an aqueous solution of HCL at concentration 0.04 mol.L-1. What is the pH at the new solution ?

1. Potassium hydroxide (KOH) is a strong base in aqueous solution. Give the pH of a KOH solution with a concentration co = 4.0 x 10-3 mol.L-1. 2. A hydrochloric acid (HCI) solution of 0.15 M concentration and volume V = 120 mL is available. 35 mL of this solution is taken and added to 100 mL of water. Calculate the concentration of all the species in solution and the pH of the new solution. 3. 100 mL of an aqueous solution of KOH at 0.01 mol.L-1 has been prepared. Give the pH of the solution. To this solution is added 50 mL of an aqueous solution of HCL at concentration 0.04 mol.L-1. What is the pH at the new solution ?

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

1. Calculate the pH of a solution prepared by mixing 27.0 mL of pure pyridine, C5H5N (d = 0.978 g/mL), with 65.0 mL of 2.75 M HCl. Kb for pyridine is 1.5 × 10-9 . 2. Calculate the pH of a solution prepared by mixing 2.15 g of butyric acid (HC4H7O2) with 0.450 g of NaOH in water. (Ka butyric acid = 1.5 × 10-5 ) 3. How many grams of potassium hydroxide KOH would have to be added to 130 mL of a 0.298 M nitrous acid HNO2, solution, in order to prepare a buffer with a pH of 3.10? (Ka = 6.0 × 10-4 )
We did an experiment in a lab. We tested for the strength of acids and bases using a conductivity test. Distilled water was used as one of the solutions. the litmus paper and phenolphthalein did not change color. It did not also conduct electricity. Hence it was assumed to be a nonelectrolyte therefore a neutral solution. However, upon searching the internet, it was found that water is not exactly acidic. A pH of 7 at 25°C represents PURE distilled water. Distilled water is considered to be slightly acidic because it absorbed carbon dioxide from the air. The pH of distilled water can range anywhere between 5.5 and 6.9, depending on how long it has been exposed to air. If this is true, then shouldn't the distilled water conduct electricity since acids conduct electricity? Yes or No? please provide an explanation and chemical equation if possible. thank you!
Buffer Preparation: Acid-Base Reactions An aqueous solution contains 0.496 M hydrocyanic acid. Calculate the pH of the solution after the addition of 2.18x10 2 moles of sodium hydroxide to 125 mL of this solution. (Assume that the volume does not change upon adding sodium hydroxide) pH = Submit Answer Retry Entire Group 8 more group attempts remaining An aqueous solution contains 0.498 M ammonia. Calculate the pH of the solution after the addition of 3.30x102 moles of hydrobromic acid to 155 mL of this solution. (Assume that the volume does not change upon adding hydrobromic acid.) pH = Submit Answer Retry Entire Group 8 more group attempts remaining Use the References to a An aqueous solution contains 0.336 M ammonia. Calculate the pH of the solution after the addition of 2.95x102 moles of hydrochloric acid to 155 ml of this solution. (Assume that the volume does not change upon adding hydrochloric acid.) pH = Submit Answer Retry Entire Group 8 more group attempts remaining
The pH of blood is 7.4. What is the ratio (to one decimal place) of bicarbonate (conjugate base) to carbonic acid (weak acid) in the blood's buffering equilibrium? Note, the K₂ of carbonic acid is 4.27 x 10-7. Write your answer this way: # to 1 Done Clear Incorrect. The ratio is 10.7 to 1, indicating that there is 10 times more bicarbonate than carbonic acid. Enter the correct answer.
This question is concerned with acid/base. The ionic product of water may be taken as 10-14 mol2dm-6. Aqueous solutions of a particular monobasic acid HX have the following pH values (see figure below). Concentration in moldm-3 PH Hydrogen ion concentration in moldm-3 Solution A 0.1 2.80 1.585 x 10-3 Solution B 0.001 3.85 Complete the table by calculating the hydrogen ion concentration of solution B. Write down the equation describing the dissociation of the acid HX in an aqueous solution.
Calculate the pH of each of the following buffered solutions. Ka(HC, HgO,)= 1.8 × 10 5 1.0.19 M acetic acid/0.29 M sodium acetate pH = 2. 0.29 M acetic acid/0.19 M sodium acetate pH = 3. 0.060 M acetic acid/0.21 M sodium acetate pH = 4. 0.21 M acetic acid/0.060 M sodium acetate pH = Visited
General Chemistry 4th Edition McQuarrie Rock Gallogly University Science Books presented by Macmillan Learning The K value for acetic acid, CH, COOH(aq), is 1.8 x 10-5. Calculate the pH of a 2.60 M acetic acid solution. pH = %3D Calculate the pH of the resulting solution when 2.50 mL of the 2.60 M acetic acid is diluted to make a 250.0 mL solution. pH = Question Source: MRG - General Chemistry Publish privacy policy terms of use contact us help about us careers N EV prime video P. II
A solution is prepared that is initially 0.095 M in propanoic acid (HC2H5CO2) and 0.31 M in potassium propanoate (KC2H5CO2). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [H3O+]. You can ieave out the M/ symbol for molanty.
Consider the following two solutions: 2.0 M Mg(NO,), and 2.0 M KCN. Which of the following statements is true? Select one: O The Mg(NO)2 solution has the same boiling point and freezing point, but a higher pH than the KCN solution. O The Mg(NO )k solution has a higher boiling point and lower freezing point than the KCN solution. O The Mg(NO,), solution has a lower boiling point and higher freezing point than the KCN solution. O The Mg(NO), solution has the same boiling point and freezing point, but a lower pH than the KCN solution. O The Mg(NO), solution has a higher boiling point and higher freezing point than the KCN solution.
A conjugate acid (HA) and its conjugate base (A") is mixed to make buffer solutions. When 0.50 mol HA and 0.50 mol A are mixed into 1.00 L solution, the pH of the solution is 4.87. Calculate the pH of the buffer solution by mixing 0.25 mol HA and 0.75 mol A into 1.00 L solution. Your pH value should have the form of XXX, XX.X, X.XX or 0.XXX.
Lareina the laboratory technician is given the task of making a solution containing HOBr (Ka=2.8×10−9) and KOBr and testing its behavior when strong acid or base is added to it. Part 1 First, Lareina combines 86.1 g KOBr and 250 mL of 1.45 M HOBr, and adds enough distilled water to make 800 mL of solution. What is the pH of this solution? pH solution = Part 2 Next, Lareina adds 12.0 mL of 2.20 M HNO3 to 360 mL of the solution made in Part 1. What is the pH of the solution after the HNO3 is added? pH after HNO3 added = Part 3 Finally, Lareina adds 10.0 mL of 2.20 M NaOH ito 365 mL of the solution made in Part 1. What is the pH of the solution after the NaOH is added? pH after NaOH added =
Lareina the laboratory technician is given the task of making a solution containing HOBr ( Ka 2.8 x 10 ) and KOBr and testing its behavior when strong acid or base is added to it. = Part 1 First, Lareina combines 81.42 g KOBr and 245 mL of 1.70 M HOBr, and adds enough distilled water to make 950 mL of solution. What is the pH of this solution? pH solution= Part 2 Next, Lareina adds 12.0 mL of 2.40 M HNO₂ to 385 mL of the solution made in Part 1. What is the pH of the solution after the HNO is added? pH after HNO, added = Part 3 Finally, Lareina 18.0 mL of 2.10 M NaOH ito 375 mL of the solution made in Part 1. What is the pH of the solution after the NaOH is added? pH after NaOH added=