A stock solution of 0.225 +/- 0.003 M NaNO2 was transferred to a 100 mL volumetric flask (class A) and diluted to the mark. If 7 mL of the stock solution was transferred using one 5-mL and two 1-mL volumetric pipettes, what is the new concentration of the solution and the uncertainty?
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A stock solution of 0.225 +/- 0.003 M NaNO2 was transferred to a 100 mL volumetric flask (class A) and diluted to the mark. If 7 mL of the stock solution was transferred using one 5-mL and two 1-mL volumetric pipettes, what is the new concentration of the solution and the uncertainty?
Given that,
Concentration of stock NaNO2 = 0.225 ± 0.003M
7 ml of stock NaNO2 is added to 100 mL volumetric flask and diluted to mark.
We have to calculate the Concentration of new NaNO2 solution with uncertainty.
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- A stock solution of 0.225 +/- 0.003 M NaNO2 was transferred to a 100 mL volumetric flask (class A) and diluted to the mark. If 7 mL of the stock solution was transferred using one 5-mL and two 1-mL volumetric pipettes, what is the new concentration of the solution and the uncertainty? Please show how to calculate the uncertainty, that is the one part I don't understand how to doYou are preparing a 100.0 mL standard solution needed for titration analysis. The NaOH (40 g/mol) pellets are measured to be 0.5341 g in a balance with acceptable uncertainty of +0.001 g. Mass of the pellets is recorded after taring the container. The pellets are put in a beaker and added with 50 ml distilled water measured by a graduated cylinder. The solution is then quantitatively transferred to a 100-mL volumetric flask with uncertainty of ±0.08 mL and diluted to a 100-mL mark. What is the concentration (M) of the solution and estimate its uncertainty by propagation? Assumption: There is no uncertainty in molar mass. Express your answer as C+/- u M.a 25.00 mL aliquot of vinegar was diluted to 250 mL in a volumetric flask. Titration of 50.00 mL aliquots of the diluted solution required an average of 34.88 mL of 0.09600 M NaOH. Express the acidity of the vinegar in terms of the percentage (w/v) of acetic acid (MM:60g/mol). Consider the correct significant figures of your answer and do not forget the unit.
- When a Vitamin C (ascorbic acid; MM = 176.12 g mol-1) tablet is crushed, dissolved and titrated with 0.0377 M KIO3(aq) to a purple/blue endpoint (given by a starch indicator), the volume of KIO3 used is 40.01 mL. How many mg of Vitamin C were in the tablet? KIO3(aq) + 5 KI + 6 H+ → 3 I2(aq) + 3 H2O I2 (aq) + ascorbic acid → 2 I- + dehydroascorbic acidIs the concentration of the solution prepared in the question below only approximate because sodium hydroxide is not a primary standard? * Find the mass in grams of sodium hydroxide that will be required to prepare a solution with a concentration of 0.500 mol·dm⁻³ in a 250 cm³ volumetric flask. [Round the answer to three decimal places. Do not type in the unit. Use a decimal point.] *1.00 grams of table salt was dissolved in 100 mL water and excess AgNO3 reagent was added and yielded 2.3789 grams of precipitate. Calculate the percentage of NaCl in the table salt. Answer must be in 2 significant figures.
- You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated cylinder and add it to a 125-mL Erlenmeyer flask. Then you add two drops of the indicator, phenolphthalein, to the oxalic acid solution in the flask. You dispense the NaOH solution from the buret into the flask (while swirling the flask) until you reach the endpoint. At the endpoint, the solution in the flask turns light pink. You repeat the titration two additional times for a total of three trials. H2C2O4 (aq) + 2 NaOH (aq) --> Na2C2O4 (aq) + 2 H2O (l) (I) (II) (III) Volume of H2C2O4 used 15.00 mL 15.00 mL 15.00 mL Molarity H2C2O4 standard solution is 0.48 M how many Moles of NaOH are there in each trial?BSA for concentration measurements is often prepared as a 10 mg/mL stock solution. Suppose you wish to prepare a series of 10 mL solutions of BSA at 1.0, 0.8, 0.6, 0.4, and 0.2 mg/mL. Using the dilution equation C1 × V1 = C2 × V2, you plan to do this by transferring a calculated volume (V1) of the 10 mg/mL (C1) into a clean test tube, then adding water in sufficient volume to produce 10 mL (V2) at the desired concentration (C2). Complete the table below, showing the volume of stock 10 mg/mL solution you need to add to each tube, and the volume of water you need to add to each. Also, convert the desired mg/mL concentration values to their equivalent in μM (micromolar; 10-6 M).A NaOH solution was titrated using potassium hydrogen phthalate (KHP, 204.22 g/mL, 99.90% purity) and phenolphthalein as indicator. Four samples of the pattern of 0.7987, 0.8039, 0.8104 and 0.8365 grams were weighed. These consumed 38.29 mL, 38.29 mL, 38.51 mL, and 39.96 mL, respectively. Calculate: A) the average molarity of the base. B) the standard deviation of the molarity and the 95% confidence limits
- During Lab 4, you are titrating a sample of new orange juice to determine its ascorbic acid (aka vitamin C) content. You have previously determined an experimental conversion factor of 0.26 mg ascorbic acid/mL dye using an ascorbic acid standard. After measuring out 5.16 mL of your orange juice sample and ~10 mL of 3% metaphosphoric acid to a graduated cylinder, you dilute the solution to 50.33 mL with DI water. You finally dispense 10.87 mL of the diluted solution into an Erlenmeyer flask, add 4 drops of HCl, and use 6.48 mL of dye to reach the equilibration point. How much ascorbic acid (mg) is in your concentrated orange juice sample? The molecular weight of ascorbic acid is 176.12 g/mol.Question 5: Find the mass in grams of sodium hydroxide that will be required to prepare a solution with a concentration of 0.500 mol·dm⁻³ in a 250 cm³ volumetric flask. [Round the answer to three decimal places. Do not type in the unit. Use a decimal point.] * The concentration of the solution prepared in Question 5 is only approximate because sodium hydroxide is not a primary standard. * A- True B- FalseA solution is prepared by mixing 20.0 mL of 0.1 00M Fe(NO3)3 with 20.0 mL of 0.00300M KSCN and 10.0 mL of DI water. Calculate the initial concentration of SCN^- in this solution? Give answer with correct amount of significant figures.