In which solution (acidic, basic, neutral water, or doesn't matter) is potassium bromide most soluble?
a. acidic
b. basic
c. neutral
d. doesn't matter
Potassium is group 2 metal and Bromide nonmetal.....group 7
I don't know that it matters.
To determine in which solution potassium bromide (KBr) is most soluble, we need to consider the solubility rules for salts.
Solubility generally depends on the interaction between the solute (KBr) and the solvent (water in this case). In this specific case, KBr is an ionic compound consisting of potassium cations (K+) and bromide anions (Br-). Water is a polar molecule, meaning it has a partial positive charge on its hydrogen atoms and a partial negative charge on its oxygen atom.
Based on the solubility rules, salts containing alkali metal cations (Group 1A in the periodic table) and halide anions (Group 7A) are typically soluble in water. Potassium (K+) is an alkali metal cation, and bromide (Br-) is a halide anion.
Therefore, potassium bromide (KBr) is expected to be soluble in water, regardless of whether the water is acidic, basic, or neutral. The solubility of KBr will remain the same because the interactions between the ions and water molecules dominate the solvation process.
So, in this case, the answer is (d) "doesn't matter." Potassium bromide would dissolve equally well in acidic, basic, or neutral water.