When preparing your unknown samples, which guideline is NOT correct? The volume of water in each sample is lower than 5 mL. The total volume of each sample is 15.00 mL Large volumes of SCN-/Fe 3+ are avoided. The volume of SCN is not larger than the volume of Fe³+.

What volume of 0.250 M HCI is required to neutralize each of the following solutions? a. 25.0 mL of 0.103 M sodium hydroxide, NaOH b. 50.0 mL of 0.00501 M calcium hydroxide, Ca(OH)2 c. 20.0 mL of 0.226 M ammonia, NH3 d. 15.0 mL of 0.0991 M potassium hydroxide, KOH

Write balanced chemical equations for the following reactions: (a) sodium oxide added to water (b) cesium carbonate added to an excess of an aqueous solution of HF (c) aluminum oxide added to an aqueous solution of HClO4 (d) a solution of sodium carbonate added to solution of barium nitrate (e) titanium metal produced from the reaction of titanium tetrachloride with elemental sodium

In each of the following cases, aqueous solutions containing the compounds indicated are mixed. Write balanced net ionic equations for the reactions that occur. (a) CaCl2 + Na3PO4 (b) iron(III) chloride and potassium hydroxide (c) lead(II) nitrate and potassium chloride

Sulfuric acid is listed in a catalog with a concentration of 95-98%. A bottle of the acid in the stockroom states that 1.00 L has a mass of 1.84 kg. To determine the concentration of sulfuric acid in the stockroom bottle, a student dilutes 5.00 mL to 500. mL She then takes four 10.00-mL samples and titrates each with standardized sodium hydroxide (c = 0.1760 M). (a) What is the average concentration of the diluted sulfuric acid sample? (b) What is the mass percent of H2SO4 in the original bottle of the acid?

When 10. L of water is added to 3.0 L of 6.0 M H2SO4, what is the molarity of the resulting solution? Assume the volumes are additive.

Chromium(III) chloride forms many compounds with ammonia. To find the formula of one of these compounds, you titrate the NH3 in the compound with standardized acid. Cr(NH3)xCl3(aq) + x HCl(aq) x NH4+(aq) + Cr3+(aq) + (x + 3) Cl(aq) Assume that 24.26 mL of 1.500 M HCl is used to titrate 1.580 g of Cr(NH3)xCl3. What is the value of x?

Vitamin C has the formula C6H8O6. Besides being an acid, it is a reducing agent. One method for determining the amount of vitamin C in a sample is to titrate it with a solution of bromine, Br2, an oxidizing agent. C6H8O6(aq) + Br2(aq) 2 HBr(aq) + C6H6O6(aq) A 1.00-g "chewable" vitamin C tablet requires 27.85 ml of 0.102 M Br2 for titration to the equivalence point. What is the mass of vitamin C in the tablet?

Consider an experiment in which two burets, Y and Z, are simultaneously draining into a beaker that initially contained 275.0 mL of 0.300 M HCl. Buret Y contains 0.150 M NaOH and buret Z contains 0.250 M KOH. The stoichiometric point in the titration is reached 60.65 minutes after Y and Z were started simultaneously. The total volume in the beaker at the stoichiometric point is 655 mL. Calculate the flow rates of burets Y and Z. Assume the flow rates remain constant during the experiment.

One method for determining the purity of aspirin (C9H8O4) is to hydrolyze it with NaOH solution and then to titrate the remaining NaOH. The reaction of aspirin with NaOH is as follows: A sample of aspirin with a mass of 1.427 g was boiled in 50.00 mL of 0.500 M NaOH. After the solution was cooled, it took 31.92 mL of 0.289 M HCl to titrate the excess NaOH. Calculate the purity of the aspirin. What indicator should be used for this titration? Why?