Q. The pH of NaOH produced after Na(s) and H₂O(l) reaction is

View solution

Q. Consider the reaction: Na(s) + H₂O → NaOH(aq) + H₂(g). Moles of H₂O required to balance the equation will be

View solution

Q. If Mg(s) is allowed to react with H₂O(l), the product other than H₂(g) will be

View solution

Q. Consider the reaction: Na(s) + H₂O(l) → NaOH(aq) + H₂(g). Moles of Na required to balance the equation are

View solution

Q. The formula MgO shows Mg oxidation number to be

View solution

Q. Consider the equation: Mg(s) + H₂O(l) → Mg(OH)₂(aq) + H₂(g). Moles of Mg(s) required to balance the equation will be

View solution

Q. When allowed to react with cold water, the element that reacts vigorously to produce H₂(g) is

View solution

Q. The element that reacts vigorously with cold water among the following is

View solution

Q. The pH of Mg(OH)₂ produced after Mg(s) and H₂O(l) reaction is

View solution

Q. Metal that reacts vigorously with cold water to produce a strongly alkaline solution is

View solution

Q. Which is incorrect about the characteristics of Group II elements?

View solution

Q. In excess water, Ca(OH)₂ produces

View solution

Q. Consider the reaction: CaO(s) + H₂O(l) → Ca(OH)₂. The state of the product in this reaction should be

View solution

Q. Upon reaction of metals of Group II with oxygen, electrons are lost more easily by

View solution

Q. The alkaline solution of Ca(OH)₂ has a pH of

View solution

Q. An increase in the nuclear charge down the Group II

View solution

Q. Upon dissolving Ca(OH)₂ in water, the solution becomes

View solution

Q. As we go down the Group-II, metals become

View solution

Q. In nature, Magnesium Oxide (MgO) is

View solution

Q. It becomes easier to lose electrons as we move

View solution