can someone please help me?
Calculate the Kb of Sodium Nitrite, NaNO2. It is the conjugate of Nitrous Acid.
Show the reaction of the base Pyridine (see bottom chart) with water.
3. What is the pH of a 0.15 M solution of the base Ethylamine?
4. What is the pH of a 0.15M monoprotic acid, HA, that is 1.25% ionized?
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can someone please help me? Calculate the Kb of Sodium Nitrite, NaNO2. It is the conjugate...
A 1.00 L solution contains 20.52 g of nitrous acid, HNO2.What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 3.56? Ka (HNO2) = 4.0 × 10–4.
How many grams of sodium nitrite, NaNO2 is required to make 1.00 L of a buffer that has a pH of 2.6? A total concentration of the acid and the salt of the conjugate base of 0.35 M is required to achieve the correct buffer capacity. Report your answers to 3 significant digits, but do NOT include units. answer is 3.74 If a buffer has a buffer capacity of 0.4 M and the concentration of the acid is 0.11 M,...
The nitrous acid/sodium nitrite conjugate pair has been chosen to prepare a buffer solution. What should the concentration ratio of NO2-/HNO2 be if the desired pH of this buffer is 4.00? (Ka of HNO2 = 4.27 x 10-4)
can someone please help me out with questions 1-5, please
To add more information this was given to me for a lab that used
a weak acid and we added a strong base through titration. We just
observed how the ph changes. Later we then used a buffer with a
weak acid to see how buffers affect ph change. These questions are
basically surrounded around those topics to help us prepare.
However, I'm kinda confused about answering them because weak...
A 1.00 L solution contains 22.52 g of nitrous acid, HNO2. What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 2.96? Ka (HNO2) = 4.0 × 10–4.
A 1.00 L solution contains 23.52 g of nitrous acid, HNO2. What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 2.36? Ka (HNO2) = 4.0 × 10–4.
A 1.00 L solution contains 15.52 g of nitrous acid, HNO2. What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 2.66? Ka (HNO2) = 4.0 × 10–4.
please help me with these questions!
At a concentration of 1 M, the weak acid HNO, is 2% ionized, and the pH of the solution is 1.7. What happens when KNO,() is dissolved into the solution? The extent of HNO, ionization The concentration of H+ The pH If a buffer solution is 0.260 M in a weak acid (K, = 6.0 x 10 ) and 0.500 M in its conjugate base, what is the pH? A 0.194 g sample of...
I've seen similar problems, but I still do not get it! Can someone show me step by step? A 34.8 mL sample of a 0.588 M aqueous nitrous acid solution is titrated with a 0.220 M aqueous sodium hydroxide solution. What is the pH after 29.9 mL of base have been added? Ka of Nitrous Acid: 3.39
could someone help me with 15.25 and 15.27 and 15.32 please?
$13 Write of the conjugate acid of substances. (The information in Tables 15.6 10/26/2019 the following substances. (The infor and 15.8 may be helpful.) (a) hydrogen sulfate ion (c) ammonia (b) water (d) pyridine he formula and name for the conjugate base of the substances. (The information in Tables 15.6 and 15.24 Writer 15.25 Write the form following substances. (The int 15.8 may be helpful.) (a) nitric acid (b)...