3. We know that pH is the negative log of the molar hydrogen ion concentration.
Thus if a HA acid molecule dissolve in water and dissociates as: HA = H+ + A- . Then pH can be determined by the following formula.
pH = —log [H+]
Given that pH = —log [1.2M]
So, from here we can conclude that the molar concentration of hydrogen ion after dissociation is 1.2M. and from this we can determine the pH of the solution also. Thus pH = -log 1.2 = —0.079.
Here we have negetive pH. any acid that yields a concentration of hydrogen ions with a molarity greater than 1 will be calculated to have a negative pH (here we have concentration of 1.2M). This is because glass pH electrodes suffer from a defect called 'acid error' which causes them to measure a higher pH than the real pH.
4. pH of a solution can be determined by negetive logarithm of the molar concentration of hydrogen ion. i.e., pH = —log [H+]
Now we have to find pH of 6.0 M HNO3 solution. Let we assume that HNO3 fully dissociates in the solution as: HNO3 = H+ + NO3-
Here 1mol HNO3 produce 1mol H+ and 1mol No3- . Thus 6M HNO3 produce 6M of H+ & 6M of NO3-.
Now pH = - log [H+]
pH = - log 6
=> pH = -0.778
So, pH of 6M HNO3 solution is -0.778.
3. (10 pts) What does the following statement represent? pH=- log (1.2 M) 4. (10 pts)...
3) (1 points) Below is a log C-pH diagram for 10" M hydrogen sulfide (H2S). (a) Label the lines with the species they represent and assign correct values to the axes. (b) Draw lines for Ht and OH on the diagram. (c) What is the pH of a solution made by mixing 10-4 M NaHS and 9x10-4 M H2S? (d) Would a solution made by adding 0.5x10-4 M Na2S and 9.5x10-4 M H2S be more acidic, more alkaline, or the...
1. Calculate the pH of the following solutions: (pH = -log (H*]) (a) 0.050 M formic acid, HCOOH, K=1.78x10-4 (b) 0.050 M hydrocyanic acid, K.-4.8x10-10 2. How would you make a 0.00025 M solution of HCI starting with 12 M solution of HCI? 3. Does the Ka for acetic acid change (within experimental tolerance) with changes in concentration? 4. What is Le Chatelier's principle? 5. What effect does the addition of acetate ions to a solution of acetic acid have...
QUESTIONS 1. Calculate the pH of the following solutions: (pH = -log[H]) (a) 0.050 M formic acid, HCOOH. K=1.78x104 (b) 0.050 M hydrocyanic acid, K.-4.8x10-10 2. How would you make a 0.00025 M solution of HCI starting with 12 M solution of HCI? 3. Does the K, for acetic acid change (within experimental tolerance) with changes in concentration? 4. What is Le Chatelier's principle? 5. What effect does the addition of acetate ions to a solution of acetic acid have...
Calculate the pH and pOH of 1.2 x 10-3 M HCl solution. Calculate pH, pOH and [OH-] of 0.1 M HNO3 solution. If a solution X has pH = 5, which of the following is true: Solution X is neutral. H3O+ ion concentration is higher than OH- concentration. c. OH- ion concentration is higher than H3O+ concentration.
U Crone (NH4CI). What is the pH of the solution? 3. (4 pts) Calculate the pH of a 0.250 M solution of potassium phenolate, KC6H50. Ka foi phenol (C6H5OH) is 1.0 x 10-10. 4. (8 pts) How do the concentration/volumes of the buffer affect the buffer capacity! E.g. 50.0 mL of 0.10 M acetic acid solution with 50.0 mL of 0.10 M sodium acetate solution vs. the buffer you made in the lab (25.0 mL of 0.10 M acetic acid...
4 questions
What is the pH of egg whites with [OH-] = 1.2 x 10-5 M? A 9.08 3.4.92 C. 11.00 D. 10.50 O E. 12.08 QUESTION 26 What is the pH of an aqueous solution contains 0.0025 M of Hydroxide ion? 2.60 3.60 10.40 11.40 8.40 A 30. mL of a 0.50M solution of NaOH is titrated with 0.50M HNO3. Calculate the pH of the solution after 30. mL of HNO3 has been added? 0.30 0.50 7.0 5.0 3.0...
pH of buffer is calculated by the equation: pH=pK, +log (base/acid). Where pK= -log Kg. For nitrous acid HONO2 Kg = 4.0.10-4; for ammonia Kg = 5.6•10-10 Determine, whether the following solution is a buffer, if yes - calculate pH for the solution, which is prepared by mixing of: 0.2 L of 0.6 M HNO2 +0.4 L 0.1 M NH3 3.00 8.77 8.67 3.10
stion 3 of 4 Calculate the pH of the solution after the addition of cach of the given amounts of 0.0683 M HNO to a 80.0 mL solution of 0.0750 M aziridine. The pKa of aziridinium is 8.04. What is the pH of the solution after the addition of 0.00 mL. HNO,? pH What is the pH of the solution after the addition of pH 5.90 mL. HNO,? What is the pH of the solution after the addition of a...
3. What is the approximate expected pH of a 0.030 M HNO, solution? What is the final pH after 1 drop (0.05 mL) of 6 M HCl is added to 1.0 L of freshly prepared pure water that was significant pH change? 4. pH of 7.0. Is there originally at a a What is the molarity of pure water at 20°C? 5. a. b. Does the concentration of water change significantly (from the value in 4-a) when enough acetic acid...
A) the pH of a 0.150 M solution of a weak monoprotic acid having Ka= 1.2×10−3 is 1.89. Find the percent dissociation of this solution. B) Find the pH of a 0.150 M solution of a weak monoprotic acid having Ka= 0.13. Find the percent dissociation of this solution.