the flask shown here contains 10.0 mL of HCl and a few drops of phenolphthalein indicator....

the flask shown here contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.140 M NaOH

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queen_honey_blossom answered 2 years ago

The flask shown here contains 10.0 mL of HCl and a few drops of phenolphthalein indicator....

The flask shown here contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.210 M NaOH.

The flask shown here contains 1.04 g of acid and a few drops of phenolphthalein indicator...

The flask shown here contains 1.04 g of acid and a few drops of phenolphthalein indicator dissolved in water. The buret contains 0.280 M NaOH. When titrated the end point of the solution is 26 mL. What volume of base is needed to reach the end point of the titration? Assuming the acid is monoprotic, what is its molar mass?

You have 5 mL of vinegar in a flask and 2 drops of phenolphthalein indicator. You...

You have 5 mL of vinegar in a flask and 2 drops of phenolphthalein indicator. You titrate exactly 36.9 mL of 0.1 mol/L NaOH from a burette directly into the flask which gives you a pale pink color. This means the solution has reached neutralization. Calculate n of the NaOH. Suppose 0.22 L of 0.5 mol/L NaOH solution was titrated with 5 L of HCl using phenolphthalein indicator. Calculate the amount of the base and the acid that were used...

Consider the three tubes below. Each contains a few drops of the color indicator bromothymol blue,...

Consider the three tubes below. Each contains a few drops of the color indicator bromothymol blue, which is yellow in acidic solutions and blue in basic solutions. One tube contains a solution of ammonium chloride, one contains ammonium acetate, and the third contains sodium acetate. Which beaker contains which salt? Explain your reasoning. 1st tube = yellow 2nd tube = green 3rd tube = blue

Kinetic Study of an Iodine Clock Reaction. Flask A contains 5.00 mL of 6 M HCl...

Kinetic Study of an Iodine Clock Reaction. Flask A contains 5.00 mL of 6 M HCl (density 1.11 g/mL). Flask B contains 5.00 mL of the same 6M HCl solution used in flask A, 2.00 mL of ethyl acetate (density 0.893 g/mL), and 3.00 mL of water (density 1.00 g/mL). Flask A was titrated with 1.00 M NaOH, and it required 31.95 mL to reach a phenolphthalein end point. Flask B was sealed and allowed to sit for 7 days...

A 10.0 mL sample of liquid bleach is diluted to 100. mL in a volumetric flask....

A 10.0 mL sample of liquid bleach is diluted to 100. mL in a volumetric flask. A 25.0 mL aliquot of this solution is analyzed using the procedure in this experiment. If 10.4 mL of 0.30 M Na2S2O3 is needed to reach the equivalence point, what is the percent by mass NaClO in the bleach? Hint: Percent by mass is grams of NaClO / mass of bleach. Presume a density for the bleach of 1.00 g/mL.

what is the molarity of a HCl solution if a 10.0 mL sample is neutralized by...

what is the molarity of a HCl solution if a 10.0 mL sample is neutralized by a 44.3 mL of a 0.111 molar solution

What is the pH after adding 10.0 mL of 0.10 M HCl to a 90.0 mL...

What is the pH after adding 10.0 mL of 0.10 M HCl to a 90.0 mL buffer solution of 0.60 M CH3COOH and 0.40 M CH3COONa at 25 °C? (Ka = 1.8 x 10−5)? What reaction will occur when HCl is added to the above buffer? 1) How many moles of acetic acid are present after the reaction? 2) How many moles of acetate ion are present after the reaction? 3) What is the concentration (in M) of acetic acid...

A 10.0 mL solution of 0.300 M NH3 is titrated with a 0.100 M HCl solution....

A 10.0 mL solution of 0.300 M NH3 is titrated with a 0.100 M HCl solution. Calculate the pH after the addition of 20.0 mL of the HCl solution. (potentially useful info: Ka of NH4+ = 5.6 x 10−10)

1. What is the change in pH when 10.0 mL of 0.010 M HCl is added...

1. What is the change in pH when 10.0 mL of 0.010 M HCl is added to 500 mL of pure water. 2. What is the change in pH when 10.0 mL of 0.010 M NaOH is added to 500 mL of pure water.

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