How many grams of KOH should be dissolved in water to make 2000.0 grams of a 10.0 ppm solution?

We need 2 * 10^-2 grams (=0.02 grams) KOH

Explanation:

Step 1: Data given

Mass of solution = 2000.0 grams

Solution = 10.0 ppm

Step 2: Calculate mass KOH needed

A solution's concentration in parts per million tells you the number of grams of solute present for every  10^6 grams of the solution.

In this case, the target solution must have a concentration of  

10.0 ppm , what means that it must contain  10.0 g  of KOH( the solute), for every  10^6 grams of the solution

This means that the mass of KOH needed to make this solution is equal to

2000 grams * 10 grams KOH/ 10^6 grams solution = 0.02 = 2 *10^-2 grams

So, if you dissolve  2 *10^-2 grams of KOH in enough water to get a total mass of the solution to  2000.0 g , you will have a  10.0-ppm  KOH solution.

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

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.