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Molar mass from atomic masses: a water molecule is H + H + O = 1 + 1 + 16 = 18 g/mol.
Grams in 1 mole of a compound: NaCl = Na + Cl = 23 + 35.5 = 58.5 g, so 1 mol of table salt weighs 58.5 g.
Molarity (M = mol ÷ L): concentration is moles of solute per litre of solution. 1 mol of salt in 2 L of water is 1 ÷ 2 = 0.50 M. Less water makes it stronger, more water makes it weaker.
Dissolved ionic compounds conduct electricity: pure water barely conducts. When NaCl dissolves it splits into Na⁺ and Cl⁻ ions that carry current between the probes. More ions per litre means more current.
Acids, bases, indicators and neutralization: red-cabbage indicator turns red in acid (vinegar), purple in neutral (water) and green in base (baking soda). An acid and a base cancel each other out mole for mole: 0.10 mol HCl needs 0.10 mol NaOH, and with 1.0 M NaOH that is mol ÷ M = 0.10 L = 100 mL. Exactly matched, the solution turns neutral (purple).