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50 mL of 0.2 M HCl, 50 mL of 0.2 NH(2) S...

`50 mL` of `0.2 M HCl, 50 mL` of `0.2 NH_(2) SO_(4)`, and `200 mL` of `0.2 M Ba (OH)_(2)` are mixed together and the volume was made to `1 L` by adding `H_(2) O`. What is the final concentration of the solution, and what is the nature of the final solution: acidic, basic or neutral?

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To solve the problem step by step, we will calculate the equivalent moles of acids and bases present in the solutions, determine the net reaction, and finally find the concentration and nature of the resulting solution. ### Step 1: Calculate the equivalent moles of HCl - Volume of HCl = 50 mL = 0.050 L - Molarity of HCl = 0.2 M - n-factor of HCl = 1 (since it donates 1 H⁺ ion) \[ ...
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