Indicate which solution in each pair has the lower pH.
(a) 0.2 M NaClO2 or 0.1 M NaClO2
(b) 0.1 M HClO2 or 0.2 M HClO2
(c) water or 0.1 M NaOH
(d) 0.1 M HF or 0.1 M HNO2
for #d values of Ka are not given for both weak Acids
Indicate which solution in each pair has the lower pH. (a) 0.2 M NaClO2 or 0.1 M...
indicate which solution in each pair has the lower pH -/0.5 POINTS No Marks. To determine what portion of the question you have correct, check question score at the top of the assignment. Indicate which solution in each pair has the lower pH. lower pH -Select--- 0.1 M HCIO 0.2 M HCIO2 0.1 M NaClO2 0.2M NACIO --Select- 0.1 M HF 0,1 M HNO2 Select 0.1 M NaOH water
Which pair of substances will form a buffer solution? OHBr, NaBr O HNO2, HCI HCI, NaOH KF, NaOH HClO2, NaClO2
2 . Without calculation , which solution in each pair has the higher pH? a) 0.10 M HNO3 or 0.10 M HNO2 ? _______________________ b) 0.10 M NaNO3 or 0.10 M NaNO2 ? _______________________ c) solution that is 0.10 M NaNO2and 0.10 M HNO2 or a solution that is 0.10 M HNO2 (only)? __________________
Calculate the pH of each two-component solution: a. 0.265 M HNO3 and 0.102 M HCN b. 0.115M NaClO2 and 0.0500M NH3 c. 0.265M HNO2 and 0.350 M NaOH
Consider a 0.2 M aqueous solution of the following. Which has the lower pH O Naci O Na2CO3 Na3PO4 Na2S
A weak acid, HA, is 0.1% ionized in a 0.2 M solution. Answer the following questions: a) What is the equilibrium constant (Ka) for the dissociation of this acid? b) What is the pH of the solution? c) How much ‘weaker’ in active acidity of the HA solution compared to 0.2 M HCl solution? d) How many mls of 0.1 M NaOH would be needed to neutralize completely 250 ml of the 0.2 M HA solution?
Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For...
The titration of 50.00 mL solution of a 0.1 M OAc- with 0.2 M HCl. OAc- is a weak base. Ka for acetic acid = 1.75 * 10^-5. a) Calculate the pH of the 50.0 mL of 0.1 M OAc- solution before the addition of any HCl. b) Calculate the pH of the resulting solution after the addition of 5.0 mL of 0.2 M HCl to the 50.0 mL of 0.1 M OAc- solution. c) Calculate the pH of the resulting...
A chemistry graduate student is given 125. mL of a 1.70 M chlorous acid (HNO2) solution. Chlorous acid is a weak acid with Ka= 1.1 x 10^-2. What mass of NaClO2 should the student dissolve in the HClO2 solution to turn it into a buffer with pH = 2.48? You may assume that the volume of the solution doesn't change when the NaClO2 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2...
1) Which of the following pairs would make suitable buffers? For each pair that does not, indicate why. (4 points) a) HS/HS b) HBr/Br c) NH4+NH, d) HC204/C2012- e) CH3NH,*/HS f) HNO/NO2 g) H2SO./HSO4 h) HF/Br 2) Which of the following pairs would make suitable buffers? For each pair that does not, indicate why. (3 points) a) 0.1 L of 1 M NH4 and 1 L of 1 M NH b) 0.1 L of 0.1 M HCL of 1 M...