A student titrates 50.0 mL of an unknown concentration of HI with 85 mL of a 1.0 M solution of NaOH to reach the equivalence point. What is the pH of the HI solution? a) 1.7 b) -0.23 c) 0.23

Consider a solution of a weak acid  being titrated with a solution of a strong base to beyond the equivalence point. Which of the following statements is incorrect?   a. The pH will increase intially and then change very little until the equivalence point is reached   b. Only a small percentage of the weak acid will react with the added base   c. The volume of the base solution required to reach the equivalence point can be less than, equal to, or more than the volume of the acid solution.   d. At the equivalence point, the solution will be basic   e. Beyond the equivalence point, the solution will be basic   f. None of the above   g. The pH of the solution in the tiration flask is affected by the total volume at any given point

A 20.00-mL sample contains 1.00 g of NAHCO,. This sample is used to standardize an NaOH solution. At the equivalence point, 39.60 mL of NaÓH have been added. K,(HCO, ) = 4.8 x 10 Indicators that change color within the pH range: bromothymol blue = 6.0 – 7.7 phenolphthalein = 8.3 – 9.8 alizarin yellow R = 10.0 – 12.0 a. What was the concentration of the NaOH? Concentration M b. What is the pH at the equivalence point? pH = c. Which indicator, bromothymol blue, phenolphthalein, or alizarin yellow R, should be used in the titration? bromothymol blue phenolphthalein allzarin yellow R y Another Version 10 item attempts remaining

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Which of the following aqueous solutions are good buffer systems?(more than one answer maybe required) a) 0.40 M sodium bromide + 0.30 M calcium bromide b) 0.25 M ammonia + 0.31 M barium hydroxide c) 0.14 M hypochlorous acid + 0.17 M sodium hypochlorite d) 0.25 M hydrochloric acid + 0.23 M potassium chloride e) 0.14 M potassium hydroxide + 0.24 M potassium chloride

When a weak acid is titrated with a strong base, at half-equivalence point, pH = ?

Calculate the Ph in the titration of 40 ml of 0.150M acetic acid by sodium hydroxide after the addition to the acid solution of: A) 15 ml of 0.150M NaOH B) 40 ml of 0.150M NaOH C) 60 ml of 0.150M NaOH :

A 34.8 mL aliquot of weak acid that has a concentration of 0.752 M will be titrated with 0.853 M NaOH. Calculate the pH of of the solution upon the addition of 0 mL of HCl. The Ka of the acid is 7.5×10-6. A 36.54 mL aliquot of weak acid that has a concentration of 0.255 M will be titrated with 0.981 M NaOH. Calculate the pH of of the solution upon the addition of 40.11 mL of NaOH. The Kb of the base is 7.9 × 10-7.

When titrating 15.0 mL of 0.10 M HCN with 0.10 M KOH, what will be the pH at the equivalence point?

A 25.0 ml sample of 1.00 M HCl is titrated with 50.0 ml of 1.00 M NaOH solution. What is the pH of this solution ? 13.5 10.5 5.52 3.06