answer:The balanced chemical equation for the reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) is: HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l) The products formed in this reaction are sodium chloride (NaCl) in aqueous state and water (H2O) in liquid state. To calculate the amount of water formed when 50 ml of 0.1 M HCl is completely reacted with 50 ml of 0.1 M NaOH, we can use the concept of moles. Moles of HCl = (Volume of HCl in L) × (Molarity of HCl) = (50 ml × 0.001 L/ml) × 0.1 M = 0.005 moles Moles of NaOH = (Volume of NaOH in L) × (Molarity of NaOH) = (50 ml × 0.001 L/ml) × 0.1 M = 0.005 moles Since the stoichiometry of the reaction is 1:1, the moles of water formed will be equal to the moles of the limiting reactant. In this case, both HCl and NaOH have the same moles, so either can be considered the limiting reactant. Moles of water formed = 0.005 moles

answer:To find the pH of a solution with a concentration of 0.1 M of hydrochloric acid (HCl), we can use the formula: pH = -log10[H+] Since HCl is a strong acid, it dissociates completely in water, releasing one H+ ion for each HCl molecule. Therefore, the concentration of H+ ions in the solution is equal to the concentration of HCl, which is 0.1 M. Now, we can plug this value into the formula: pH = -log10(0.1) pH = -(-1) pH = 1 So, the pH of the solution is 1.

answer:The balanced chemical equation for the reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) to form sodium chloride (NaCl) and water (H2O) is: HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)

answer:The balanced chemical equation for the reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) is: HCl + NaOH → NaCl + H2O This is an acid-base neutralization reaction, where hydrochloric acid donates a proton (H+) to sodium hydroxide, which donates a hydroxide ion (OH-). The products are sodium chloride (NaCl) and water (H2O). In a neutralization reaction, the concentration of H+ and OH- ions in the resulting solution depends on the initial concentrations of the acid and base. If the reaction goes to completion and both reactants are present in stoichiometric amounts, the resulting solution will be neutral, with a pH of 7. In this case, the concentration of H+ and OH- ions will be equal to 1 x 10^-7 M, as this is the concentration of these ions in pure water at 25°C. If there is an excess of either the acid or the base, the concentration of H+ or OH- ions in the resulting solution will be different. To determine the exact concentration, you would need to know the initial concentrations of the reactants and the volume of the solution.