which of the following would form acidic,basic or neutral solutions:nh4f,nh4cn,nh4ch3coo,nh4cl,ba(ch3coo)2,nacn,caso4,cr(no3)3,fecl3,na2co3
To determine whether a compound would form an acidic, basic, or neutral solution, we need to analyze the nature of the ions formed when the compound dissociates in water.
1. NH4F:
When NH4F dissolves in water, it dissociates into ammonium (NH4+) and fluoride (F-) ions. NH4+ is a weak acid, and F- is the conjugate base of a weak acid. Therefore, NH4F would form a slightly acidic solution.
2. NH4CN:
NH4CN dissociates into ammonium (NH4+) and cyanide (CN-) ions. Similar to NH4F, NH4+ acts as a weak acid. However, CN- is the conjugate base of a weak acid. Therefore, NH4CN would also form a slightly acidic solution.
3. NH4CH3COO:
NH4CH3COO dissociates into ammonium (NH4+) and acetate (CH3COO-) ions. NH4+ acts as a weak acid, while CH3COO- is the conjugate base of a weak acid. However, in this case, acetate is a relatively strong base compared to fluoride or cyanide. As a result, NH4CH3COO would produce a slightly basic solution.
4. NH4Cl:
When NH4Cl dissolves in water, it dissociates into ammonium (NH4+) and chloride (Cl-) ions. NH4+ acts as a weak acid, while Cl- is the conjugate base of a strong acid. Since the Cl- ion does not undergo hydrolysis, NH4Cl would produce a neutral solution.
5. BA(CH3COO)2:
BA(CH3COO)2 dissociates into barium (Ba2+) and acetate (CH3COO-) ions. Ba2+ does not undergo hydrolysis, and CH3COO- acts as a weak base. Thus, BA(CH3COO)2 would produce a slightly basic solution.
6. NaCN:
NaCN dissociates into sodium (Na+) and cyanide (CN-) ions. Na+ does not undergo hydrolysis, and CN- is the conjugate base of a weak acid. Hence, NaCN would form a slightly basic solution.
7. CaSO4:
CaSO4 dissociates into calcium (Ca2+) and sulfate (SO4 2-) ions. Neither Ca2+ nor SO4 2- undergo hydrolysis. Therefore, CaSO4 would produce a neutral solution.
8. Cr(NO3)3:
Cr(NO3)3 dissociates into chromium (Cr3+) and nitrate (NO3-) ions. Neither Cr3+ nor NO3- undergo hydrolysis. Thus, Cr(NO3)3 would form a neutral solution.
9. FeCl3:
FeCl3 dissociates into iron (Fe3+) and chloride (Cl-) ions. Similar to Cr(NO3)3, neither Fe3+ nor Cl- undergo hydrolysis. Hence, FeCl3 would produce a neutral solution.
10. Na2CO3:
Na2CO3 dissociates into sodium (Na+) and carbonate (CO3 2-) ions. Na+ does not undergo hydrolysis, but CO3 2- acts as a strong base. Consequently, Na2CO3 would form a basic solution.
Remember, this explanation is based on the assumption that all compounds are dissolved in water. The term "slightly acidic" or "slightly basic" suggests that the pH of the solution would be closer to neutral but leaning toward the respective acidic or basic side.