Concept explainers
(a)
Interpretation:
To explain whether
Concept introduction:
As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all the amphiprotic species have hydrogen atom.
(b)
Interpretation:
To explain whether
Concept introduction:
As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all the amphiprotic species have hydrogen atom.
(c)
Interpretation:
To explain whether
Concept introduction:
As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all the amphiprotic species have hydrogen atom.
(d)
Interpretation:
To explain whether
Concept introduction:
As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all the amphiprotic species have hydrogen atom.
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EBK GENERAL CHEMISTRY
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- Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. CH:NH2(aq) + HCIO:(aq)- |3- 2- 4- 2+ |3+ 4+ 1 2 3 4 5 6 7 8 O2 O3 D4 Os |1 6. 10 (s) (1) (g) (aq) + H2O H3O+ H CI OH- C Reset x H2O Deletearrow_forwardIt turns out that Ba(OH)2 is also considered a strong base. What is the [OH-] concentration in 0.34 M Ba(OH)2(aq) solution?arrow_forwardWhat molarity of Ag+ ions is required for the formation of a precipitate in 1.0 × 10-5 M NaCl(aq)?arrow_forward
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