dditional Problems. Show all work using dimensional analysis using correct sig figs and units. A 25.00 mL sample of barium hydroxide requires 23.55 mL of 0.2550 M hydrochloric acid to reach the titration end point. Calculate the molar concentration of the barium hydroxide solution. 2HCl(aq) + Ba(OH)2(aq) → BaCl2 (aq) + 2H2O(1) 'hat mass, in grams, of sodium chloride is needed to prepare 5.0 mL of 10%(m how all work using dimensional analy

You are given four different aqueous solutions and told that they each contain NaOH, Na2CO3, NaHCO3, or a mixture of these solutes. You do some experiments and gather these data about the samples. Sample A: Phenolphthalein is colorless in the solution. Sample B: The sample was titrated with HCl until the pink color of phenolphthalein disappeared, then methyl orange was added. The solution became pink. Methyl orange changes color from pH 3.01 (red) to pH 4.4 (orange). Sample C: Equal volumes of the sample were titrated with standardized acid. Using phenolphthalein as an indicator required 15.26 mL of standardized acid to change the phenolphthalein color. The other sample required 17.90 mL for a color change using methyl orange as the indicator. Sample D: Two equal volumes of the sample were titrated with standardized HCl. Using phenolphthalein as the indicator, it took 15.00 mL of acid to reach the equivalence point; using methyl orange as the indicator required 30.00 mL HCl to achieve neutralization. Identify the solute in each of the solutions.

According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?

The amount of oxygen, O2, dissolved in a water sample at 25 C can be determined by titration. The first step is to add solutions of MnSO4 and NaOH to the water to convert the dissolved oxygen to MnO2. A solution of H2SO4 and KI is then added to convert the MnO2 to Mn2+, and the iodide ion is converted to I2. The I2 is then titrated with standardized Na2S2O3. (a) Balance the equation for the reaction of Mn2+ ions with O2 in basic solution. (b) Balance the equation for the reaction of MnO2 with I in acid solution. (c) Balance the equation for the reaction of S2O32 with I2. (d) Calculate the amount of O2 in 25.0 mL of water if the titration requires 2.45 mL of 0.0112 M Na2S2O3 solution.

Strong acid solutions may have their concentration determined by reaction with measured quantities of standard sodium carbonate solution. What mass of Na2CO3 is needed to prepare 250. mL of 0.0500 M Na2CO, solution?

A student carries out the following titration by adding H2SO4 drop-wise to a solution of Ba(OH)2.H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2H2O(l)The conductivity of the reaction mixture __  as H2SO4 is added until the equivalence

A technician would like to standardize an unknown Ca(OH)2 solution. It takes 18.53 mL of a 0.174 M solution of HCI to titrate 25.00 mL the unknown Ca(OH)2 solution. Calculate the molarity of the Ca(OH)2 solution. Tip: Don't forget to consider the mole ratio between HCl and Ca(OH)2. 2 HCI (aq) + Ca(OH), (aq) CaCl2 (aq) + 2 H2O (1)

Potassium hydrogen phthalate, known as KHP (molar mass = 204.22 g/mol), can beobtained in high purity and is used to determine the concentration of solutions ofstrong bases by the reactionHP −(aq) + OH −(aq) → H2O(l) + P2 −(aq)If a typical titration experiment begins with approximately 0.5 g KHP and has a finalvolume of about 100 mL, what is an appropriate indicator to use? The pKafor HP−is5.51.

It takes 38.65 ml of a 0.0895 M hydrochloric acid solution to reach the equivalence point in the reaction with 25 mL of barium hydroxide. 2HCI(aq) + Ba(OH)2(aq) --> 2H20(1) + BaCl2(aq) What is the molar concentration of the barium hydroxide solution?

5.0-mL sample of 0.100M HCl(aq) is titrated with 0.125M NaOH. How many milliliters of NaOH will be needed to reach the endpoint? HCl(aq) + NaOH(aq) → NaCl(aq) H 2 O(l)