A beaker containing 500.0 mL was determined to contain 0.150 M ammonia (NH3) and 0.150 M ammonium chloride NH4 To this solution was added 50.0 mL of 0.15 M hydrochloric acid (HCl). What was the change in pH of the ammonia, ammonium ion solution?

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A: Molarity is defined as number of mole of solute divide by volume of solution in liter

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Q: A 100.0 mL solution of NaOH reaches the equivalence point when 39.79 mL of a 0.0300 M solution of…

A: GivenVolume of NaOH= 100.0mLVolume of HCl= 39.79 mLMolarity of HCl= 0.03M

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Q: What was the concentration of the weak acid?

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Q: A 35.7 mL sample of a 0.324 M aqueous acetic acid solution is titrated with a 0.422 M aqueous sodium…

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Q: If 316.0 mg of AgBr is completely dissolved in 144.0 mL of 0.12 M NH3, what is the equilibrium…

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Q: A 32.4 mL sample of a 0.432 M aqueous hydrofluoric acid solution is titrated with a 0.399 M aqueous…

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Q: At what point in the titration have you reached when 40.0 mL of 0.250 M KOH has been added to 45.0…

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Q: It took 24.37 mL of 0.1224 M NaOH to reach the endpoint when titrating a sample containing 0.1650g…

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Q: A 10.0mL vinegar sample was mixed with 60mL of water in a flask, phenolphthalein was added, and it…

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Q: How many litres of 0.265 mol/L solution of phosphoric acid are necessary to completely neutralize…

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Q: In the experiment conducted to determine the amount of acetic acid in vinegar, 8.2 mL of a 0.098 M…

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Q: A 31.8 mL sample of a 0.528 M aqueous acetic acid solution is titrated with a 0.422 M aqueous sodium…

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Q: Consider an analyte solution of 50.0 mL of 0.050 M hydrochloric acid, HCl, titrated against 0.10 M…

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Q: By titration, it is found that 36.7 mL of 0.117 M NaOH(aq) is needed to neutralize 25.0 mL of…

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Q: A 37.6 mL sample of a 0.369 M aqueous nitrous acid solution is titrated with a 0.240 M aqueous…

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Q: A 21.0 mL sample of a 0.433 M aqueous nitrous acid solution is titrated with a 0.442 M aqueous…

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.