Which of the following statements is/are true? I: The conjugate acid of C6H5NH2 is C6H5NH3+ II: An acid with Ka = 1x10−3 is stronger than an acid with Ka = 1x10−4 III: A strong acid will be completely dissociated at equilibrium A) Only I B) Only II C) I and III D) II and III E) I, II, and III

E. I, II, and III.

Explanation:

I. C6H5NH2 + H2O --> C6H5NH3^+ + OH-

C6H5NH2 is a weak base means it is a good proton donor (strong conjugate acid).

II. Any aqueous acid with a pKa value of less than 0 is almost completely deprotonated and is considered a strong acid.

pka1 = - log[1 x 10^-3]

= 2

pka1 = - log[1 x 10^-4]

= 3

pka1 is a stronger acid.

III. A strong acid will be completely dissociated at equilibrium.

uranium-238 i believe is your answer

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.