Answer:
Don’t change, keep the same
Explanation:
Answer:
B is true.
Explanation:
A buffer is the mixture of a weak acid with its conjugate base or vice versa.
An effective buffer has a pH of pKa ± 1. Using H-H formula:
pH = pKa + log [base] / [acid]
1 = log [base] / [acid]
10 = [base] / [acid]
Or
-1 = log [base] / [acid]
0.1 = [base] / [acid]
<em>In other words, the </em>1 [base] / [acid] ratio in an effective buffer is between 0.1-100. <em>A IS FALSE</em>
The buffer is most resistant to pH change when pH = pKa. Using H-H formula:
pH = pKa + log [base] / [acid]
0 = log [base] / [acid]
1 = [base] / [acid]
<em>In other words, when [base] = [acid] </em><em>B IS TRUE</em>
<em />
In a buffer, an effective buffer must have a higher concentration of pair acid conjugate base. Thus <em>C IS FALSE</em>
The addition of strong base produce conjugate base decreasing concentration of acid. Too much strong base produce a big [base] / [acid] ratio destroying buffer. <em>D IS FALSE</em>
True, the bigger the object the more thermal energy it can hold.
Mary could do two types of experiments
<em>Type 1</em>. She could <em>hold the cation constant and vary the anion</em>.
She could try solutions of NaCl, NaBr, NaI, Na₂SO₄, Na₃PO₄, etc.
These experiments would tell her which <em>anions</em> are the best conductors.
<em>Type </em>2. She could <em>hold the anion constant and vary the cation</em>.
She could try solutions of NaNO₃, KNO₃, Mg(NO₃)₂, Ca(NO₃)₂, Al(NO₃)₃, etc.
These experiments would tell her which <em>cations</em> are the best conductors.
