is kbro4 an acid or base?
318118
KBrO4 is a salt. It is neither an acid nor a base, and it does not hydrolyze to form an acidic or basic solution. It can be formed from the reaction of an acid and a base.
985318
N a X 2 H P O X 4 is amphoteric, which means it can act as a base or as a acid depending on which substance they react with. ✨A salt formed between a weak acidand a weak base can be neutral,acidic, or basic depending on the relative strengths of the acid and base.
1145685
It is a salt of a strong acid ( H2SO4) and strong base ( Ca(OH)2 ). ... It's slightly basic because H2SO4 is a strong acid but HSO4(-) isn't: the bisulphate ion has a measurable acidity constant, albeit comparatively large. Thus the sulphate ion SO4(=) is a weak base.
781022
HPO4–2 can accept two protons further(and becomes phosphoric acid, H3PO4), so according to Bronstd-Lowry theory it is an base. And also it can donate the last proton it i having to become phosphate ion,PO4–3, so it is acid also. practically there are many species that can act as both acids and base.
230573
Ethers serve as Lewis bases and Bronsted bases. Strong acids protonate the oxygen to give "oxonium ions". For instance, diethyl ether forms a complex with boron trifluoride, i.e. diethyl etherate (BF3·OEt2).
209845
HSO4- is an acidic anion because it tends to donate protons when in pure water. Notice how the first arrow is not an eqilibrium - it fully dissociates and the second only partially so some of the HSO4- will donate protons. Only in a very acidic environment would HSO4- act as a base.
450511
If you see any other acid or base than one of these strong ones it will be a weak acid or base (unless I specifically say otherwise in the problem). The 7 common strong acids are: HCl, HBr, HI, HNO3, HClO3, HClO4 and H2SO4 (1st proton only).
34566
Acidity/basicity Ionic compounds containing hydrogen ions (H+) are classified as acids, and those containing electropositive cations and basic anions ions hydroxide (OH−) or oxide (O2−) are classified as bases. Other ionic compounds are known as salts and can be formed by acid–base reactions.
687219
Metal hydrides, metal oxides, and metal hydroxides are bases. Nonmetal hydrides, nonmetal oxides, and nonmetal hydroxides are acids. The acidic hydrogen atoms in the non-metal hydroxides in the table above aren't bound to the nitrogen, sulfur, or phosphorus atoms.
474894
General base dissociation in water is represented by the equation B + H2O --> BH+ + OH-. Ka and Kb values measure how well an acid or base dissociates. Higher values of Ka or Kb mean higher strength. General Ka expressions take the form Ka = [H3O+][A-] / [HA].
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Ca(OH)2 is a strong base. A strong base is something like sodium hydroxide or potassium hydroxide which is fully ionic. You can think of the compound as being 100% split up into metal ions and hydroxide ions in solution.
701904
Aluminium hydroxide is amphoteric. In acid, it acts as a Brønsted–Lowry base. It neutralizes the acid, yielding a salt: 3 HCl + Al(OH)3 → AlCl3 + 3 H2O.
999989
NH4NO3 is an acid. Its pH is around 5.4. If a substance has a pH lower than 7, it is an acid. If its pH is higher than 7, it is a base.
735181
In terms of its acid–base properties, chloride is a very weak base as indicated by the negative value of the pKa of hydrochloric acid. Chloride can be protonated by strong acids, such as sulfuric acid: NaCl + H2SO4 → NaHSO4 + HCl. Ionic chloride salts reaction with other salts to exchange anions.
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According to the Brønsted-Lowry acid base-theory, an acid is a proton (hydrogen ion, H+ ) donator, and a base is a proton (hydrogen ion, H+ ) acceptor. Ammonia is the hydrogen ion acceptor, and is therefore a base, and water is the hydrogen ion donor, and is therefore an acid.
146754
Because DMSO is only weakly acidic, it tolerates relatively strong bases and as such has been extensively used in the study of carbanions. A set of non-aqueous pKa values (C-H, O-H, S-H and N-H acidities) for thousands of organic compounds have been determined in DMSO solution.
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The drug in Figure 3.4 contains a phenol, a secondary alcohol, and a tertiary amine. Only the phenol and tertiary amine are ionizable functional groups. The pKa values for each of these functional groups were found in the appendix of "The Textbook of Organic, Medicinal and Pharmaceutical Chemistry, 10th edition".