If a student used the molar mass of magnesium to calculate the concentration in parts per million (ppm) of a manganese stock standard solution, would the reported weight percent of manganese in a subsequent unknown, that was compared colorimetrically, be higher, lower, or not change?
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If a student used the molar mass of magnesium to calculate the concentration in parts per million (ppm) of a manganese stock standard solution, would the reported weight percent of manganese in a subsequent unknown, that was compared colorimetrically, be higher, lower, or not change?
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- On the redox titration experiment, Standardization of Na2S2O3 with KIO3 standard solution, what can be replaced KIO3 to make safer solvent and auxiliaries( reduced toxic waste)? explain why?To keep ionic strength constant and maintain a more consistent matrix in a solution where ions could be influencing each other, another component is often added to the solution This is an ionic compound, not involved directly with the reaction, called an ionic strength adjuster (ISA) ingredient. What is the ionic strength, μμ, of a solution that contains 0.0280 M (NH4)2SO4 as the ISA ingredient?A titrant solution of KMnO was standardized with 0.2000 grams of Na2C2O4 and consumed 27.75 mL to reach end point. Calculate the standardized NORMAL concentration of the titrant.
- A titrant solution of KMNO4 was standardized with 0.2g of Na2C2O4 amd consumed 27.75 mL to reach endpoint. What is the standardized normal concentration of the titrant?How do we keep relative supersaturation low by controlling solute concentration? concentration should be constant concentration should be higher concentration should be lower concentration should be fluctuatingHow to prepare these solutions? 250.0 mL 0.125 M stock Na2S2O3 solution from Na2S2O3·5H2O crystals 250 mL 0.10 M NaOHNOTE: Use the 1.0 M NaOH prepared250.0 mL standard 2500 ppm Cu(II) stock solutiona. Weigh and dissolve appropriate amount of Cu(NO3)2·5H2O crystals in enough distilled water.
- What is the concentration of Cu2+ in a 1 mL solution taken from a 10 mL solution of (1) 0.040 M in CuSO4 and 0.050 M in tartrate(2) 0.040 M in CuSO4 and 0.100 M in tartrate(3) 0.040 M in CuSO4 and 0.150 M in tartrate all with distilled water (to equal the 10 mL)To prepare a stock solution of EDTA, 73 grams of EDTA were mixed to 500 mL of distilled water. What is the: A. Molar concentration of EDTA stock solution is Blank 1M Using the prepared EDTA stock solution above, 25 mL of 200 mM working solution has to be made. Calculate for the following: B. Volume of EDTA stock solution to be diluted is Blank 2mL C. Volume of distilled water is Blank 3mL1. A 1.2-gram sample of lanolin was treated with Wij’s solution and excess potassium iodide solution. The liberated iodine reacted with 30 ml of 0.1 N sodium thiosulfate solution. If the iodine value was determined as 12.69, what is the volume used in blank titration? 2. A fat sample with combination of acids contain standard hydrochloric acid for blank and sample with 8mL and 5mL respectively. The normality of the standard hydrochloric acid is 0.93N and the weight of the sample is 3 grams. Calculate the saponification value. 3. A 3.50-gram sample of Streptomycin powder was tested for its water content. If the water equivalence factor of the KF reagent was 4.6, what is the percentage water content of the sample if 9.2 ml of the KF reagent was used? 4. A 500mg oil sample is taken from a conical flask and is dissolved in 50mL distilled alcohol. An indicator is added and is then titrated against 0.112N KOH until a slight pink color appears. It took 17.6mL of the titrant to reach the…
- (b) Using appropriate chemical reactions for illustration, show how calcium present as the dissolved HCO3- salt in water is easier to remove than other forms of hardness, such as dissolved CaCl2. (c) A water has the following analysis: mg/l mg/l Na+ - 20 Cl- - 40 K+ - 30 HCO3- - 67 Ca2+ - 5 CO32- - 0 Mg2+ - 10 SO42- - 5 Sr2+ -2 NO3- - 10 What is the total hardness, carbonate hardness and noncarbonated hardness in mg/l as CaCO3.Suppose a standard vitamin C solution has a concentration of 0.0125 M. You measure out 20.00 mL of this vitamin C standard solution, and 38.62 mL of I2 solution is required to standardize the solution. What is the standardization factor of this iodine solution?A student weighted a 1.150gram sample of pure KHP and titrated it with 36.45ml of KO solution. Calculate the normality of the KOH.