Astudent is asked to determine the molarity of a strong base by titrating it with 0.250 m solution of h2so4. the students is instructed to pipet a 20.0 ml portion of the strong base solution into a conical flask, to add two drops of an indicator that changes at ph = 7, and to dispense the standard h2so4 solution from a buret until the solution undergoes a permanent color change. the initial buret reading is 5.00 ml and the final reading is 30.00 ml at the equivalence point. what is the [oh-] in the strong base solution? 0.313 m0.750 m0.375 m0.625 m

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.

the answer is barium and copper bromide