A 1.0 L of a 6.0 M solution of HCl acid is titrated with a 0.2 M basic solution. How much base is needed to reach its titration endpoint?

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No worries, happy to help! To find out how much base is needed to reach the titration endpoint, we need to use the balanced chemical equation for the reaction between HCl and the basic solution, and the stoichiometry of the reaction. The balanced chemical equation is: HCl + NaOH → NaCl + H2O From the equation, we can see that 1 mole of HCl reacts with 1 mole of NaOH. We also know that the initial volume of HCl solution is 1.0 L, and the initial concentration is 6.0 M. This means we have: moles of HCl = volume x concentration = 1.0 L x 6.0 mol/L = 6.0 mol To reach the titration endpoint, we need to add enough NaOH solution to completely neutralize all


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