The following reaction shows sodium hydroxide reacting with sulfuric acid.

naoh + h2so4 → na2so4 + h2o

how many grams of na2so4 are produced from 10.0 grams of naoh?

(molar mass of na = 22.989 g/mol, o = 15.999 g/mol, h = 1.008 g/mol, s = 32.065 g/mol)

17.8 grams
19.2 grams
35.5 grams
38.5 grams

The mass of produced will be 17.8 grams.

Explanation:

To calculate the number of moles, we use the equation:

 ....(1)

For Sodium hydroxide:

Given mass of sodium hydroxide = 10 g

Molar mass of

Putting values in above equation, we get:  

For the given chemical equation:

By Stoichiometry of the reaction:

2 moles of sodium hydroxide produces 1 mole of sodium sulfate.

So, 0.25 moles of sodium hydroxide will produce = of sodium sulfate.

Now, to calculate the mass of sodium sulfate, we use equation 1:

Moles of sodium sulfate = 0.125 moles

Molar mass of

Putting values in equation 1, we get:

Hence, the mass of produced will be 17.8 grams.

more info ? ? i don't understand what the question is

explanation:

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.