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To tell if Na2SO4 (Sodium sulfate) forms an acidic, basic (alkaline), or neutral solution we can use these three simple rules along with the neutralization reaction that formed Na2SO4 . First...
12 Ιουλ 2019 · Example \(\PageIndex{3}\): Determining the Acidic or Basic Nature of Salts. Determine whether aqueous solutions of the following salts are acidic, basic, or neutral: KBr; NaHCO 3; NH 4 Cl; Na 2 HPO 4; NH 4 F
A salt that is derived from the reaction of a strong acid with a strong base forms a solution that has a pH of 7. An example is sodium chloride, formed from the neutralization of \(\ce{HCl}\) by \(\ce{NaOH}\). A solution of \(\ce{NaCl}\) in water has no acidic or basic properties, since neither ion is capable of hydrolyzing.
Predict whether aqueous solutions of these compounds are acidic, basic, or neutral. \(\ce{KNO_3}\) \(\ce{CrBr_3} cdot \ce{H_2O}\) \(\ce{Na_2SO_4}\) Given: compound. Asked for: acidity or basicity of aqueous solution. Strategy: Assess the acid–base properties of the cation and the anion.
5 Σεπ 2015 · When I have a solution of $\ce{Na2SO4}$, the sodium sulfate should ionize: $$\ce{Na2SO4(aq) -> 2Na+(aq) + SO4^{2-}(aq)}$$ In my mind, the sodium ions should just float around, but because $\ce{HSO4-}$ is a weak acid:
If only the cation reacts with water, the solution will be acidic. If only the anion reacts with water, the solution will be basic. If both species react with water, the pH of the solution will depend on the relative strengths of the cation and the anion.
16 Αυγ 2016 · However, according to Wikipedia as well as my teacher, sodium sulfate $\ce{Na2SO4}$ is neutral, but Wikipedia also says the acidic hydrogen on the bisulfate ion has $\mathrm{p}K_\mathrm{a} \approx 2$, so sulfate would have $\mathrm{p}K_\mathrm{a} \approx 12$ and a $1\ \mathrm{M}$ solution of sulfate with a perfectly non-acidic counterion would ...
