1. List all the strong aqueous acids. What is the difference between a strong ac
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1. List all the strong aqueous acids. What is the difference between a strong acid and a weak acid? How do the concentrations of the strong and weak acids compare to the H3O+ in solution? You don't need to list all of the strong aqueous acids. I am guessing strong acid has more hydrogen ions? 2. What is pH? What happens to pH as the [H3O+] increases? Support your answer by comparing the pH of 0.50 M and 0.050 M HCl. For this one I know ph is the measurement of the acidity/baic of the solution 3. Why is the pH of basic solution greater than 7.0 while that of acids is less than 7.0? Would the pH of a 0.1 M weak acid be greater than or less than that of a 0.1 M strong acid ? 4. If the measured pH of a 0.10 M weak acid, HA, is 2.45, what is its experimental Ka value. 5. Give examples of a neutral salt, acidic salt and basic salt. Explain your choice.Explanation / Answer
1. Acids and bases may be very strong or weak. Strength refers to how well an acid or base separates into ions in water. In a strong acid, most of the molecules break up into solutions. In a weak acid, fewer molecules break up into ions.
A strong acid is an acid which ionises almost completely when dissolved in water to produce a high concentration of hydrogen ions.
A weak acid is an acid which partially ionises when dissolved in water to produce a low concentration of hydrogen ions.
("Strong" and "weak" don't really refer to the power of the acid in question. One of the most hazardous acids of all is hydrofluoric acid, which is a weak acid.)
2."H+" doesn't exist as such in water - H3O+ (the hydronium ion) is present. And we often represent this ion as "H+(aq)". So it's strictly this ion that is referred to in pH calculations, but for the sake of saving a moment's time we regularly write [H+].
A pH change of 2 corresponds to a change of a hundredfold in the concentration of "H+(aq)
3.Acidic solutions have pH values less than seven, whereas basic ones have pH readings greater than seven. A pH value of 7 is considered neutral.
Solutions that are neither very acidic nor very basic have pH values between 2 and 12. Solutions with pH values below 2 are very acidic, and those with pH values above 12 are very basic.
Note that the pH scale is not linear; it is logarithmic. A change in pH from 3 to 4 or from 8 to 9 represents a tenfold decrease in acidity (or increase in alkalinity). Hence, going from 3 to 5 represents a 100-fold decrease in acidity.
5.Acidic Salt :
NH4Cl ( Ammonium chloride ) -- Salt of Weak Base & Strong Acid
NaH2PO4 ( Sodium dihydrogenphosphate )
Basic Salt :
Na2CO3 ( Sodium carbonate ) -- Salt of Weak Acid & Strong Base
Na3PO4 ( Trisodium phosphate )
Neutral Salt :
NaCl ( Sodium chloride )
Na2SO4 ( Sodium sulfate )
KNO3 ( Potassium nitrate )
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