Please answer these question:
_ H2S is a stronger acid than phosphene ,PH3. What may you conclude about the strengths of their conjugate bases? Explain.
_Give examples of ions which can act as an acid or as a base, writing net ionic equations for each. Are they Amphiprotic or Amphoteric? Explain.
The conjugate base of weak acid is strong and the conjugate base of strong acid weak.
Therefore, The conjugate base(PH2-) of weak acid phosphene ,PH3 is strong
The conjugate base(SH-) of strong acid H2S, is weak
The examples of ions which can act as an acid or as a base are H2PO4-, HPO42-, HSO4-
A pair of substances which differ by H+ ion are called conjugate acid -base pair.
The net ionic equations are
i) H2PO4- -------> H+ + HPO42- acid base
H2PO4- + H+ ---------------> H3PO4 base acid
ii) HPO42- ----------> H+ +
PO43-
acid base
HPO42- + H+ ---------> H2PO4-
base acid
iii) HSO4- + H+ ---------> H2SO4
acid base
HSO4- ---------------> H+ + SO42-
base acid
Amphiprotic and Amphoteric are same
Amphiprotic solvents act both as protophilic or protogenic, e.g., water, ammonia, ethyl alcohol etc
H2O + H+ ---------------> H3O+ H2O ------------------> OH- + H+
base acid acid base
Please answer these question: _ H2S is a stronger acid than phosphene ,PH3. What may you conclude about the strengths of...
Chem 1030 Chapter 16 Chemistry of Acids and Bases 4. Predict the stronger acid in each pair and explain why. a) H3P or HAs b) H3P or HS c) H2SeO4 or H2Se03 d) HOCN or HCN (In HOCN, the H ion is attached to the O atom of the OCN ion.) 5. The conjugate bases for the acids F3CCOOH and H;CCOOH are shown.:03.0: 0 0 : a) Which conjugate base is stronger, i.e. which is more readily accept a proton?...
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please help l, will rate! thabk you!! Why does a solution of a weak acid and its conjugate base act as a better buffer than does a solution of the weak acid alone? The presence of both the acid and the base provides a significant concentration of both an acid and a base, making it harder to change the pH A solution of a weak acid alone has no base present to absorb added acid. The presence of both the...
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