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- Standardization of a sodium hydroxide (NaOH) solution against potassium hydrogen phthalate (KHP) yielded the following results: Mass of KHP, g Volume of NaOH, mL 0.7987 38.29 0.8365 38.96 0.8104 38.51 0.8039 38.29 MM KHP: 204.22 MM NaOH: 40.00 a. Calculate the mean molar concentration of sodium hydroxide. (First, compute the concentration of NAOH in each titration then compute for its mean/average value.) b. Calculate the standard deviation. Please provide solutions for your answers. If you have used your calculator for calculating for mean and standard deviation, you can just provide the formula with the values indicated.3. The following molarities were calculated from replicate standardizations of a NaOH solution: 0.502 8, 0.502 9, 0.502 3, 0.503 1, 0.502 6, 0.502 7, 0.503 4, and 0.502 5. Assuming no systematic errors, within what range are you 90% certain that the true mean value of the molarity falls?KMnO4 and Na2C2O4 solutions were used in the reactions that took place in a back titration to determine the amount of H2O2 in a sample. Calculate the concentration of H2O2 in the sample (w / v) as% by making appropriate assumptions for the volumes and normality of all these solutions.
- (a) A solution of 20.91 % by weight H₂SO4, has a specific gravity of 1.150. What is the normality of this solution? (b) Water is added to dilute this solution to a solution of 3.03% by weight H2SO4 (SG=1.020). What is the new normality of the resulting solution and how were they mixed? (Assume 100 mL of the original solution was used.)Reagent nitric acid is 67.74% HNO3 by mass and its molarity is 14.33 M. Calculate the mole fraction of nitric acid in the solution. Express final answer with two decimal places.An experiment was performed to look at how density changes when t he ratio of water and ethanol was changed. The following data was obtained: % Mass Ethano1.00 2.50 3.50 4.00 6.00 7.50 9.50 Density, g/mL0.9963 0.9936 0.9918 0.9910 0.9878 0.9855 0.9826 Use Excel or a similar spreadsheet program to plot these six data points and answer the following questions . a.What is the independent variable? b.What is the dependent variable? c.What is the equation of the best-‐fit line? d.What is the value of the coefficient of determination? e. According to the best-‐fit line, what should the density of pure water be (i.e. what is the density when % mass ethanol = 0.00)?
- A 25mL volumetric pipet is used to deliver a sample of the stock solution marked “0.6000M X2SO4” into a 100mL volumetric flask. Distilled water is added to the flask until it is about 3/4thfull, the solution is mixed well, then more water is added to fill it up to the calibration mark, then it is mixed again. Calculate the concentration of X+ion in the dilute solution made above.A chemist mixes 49. g of chloroform with 53. g of acetyl bromide and 29. g of acetone. Calculate the percent by mass of each component of this solution. Be sure each of your answer entries has the correct number of significant digits. component mass percent x10 chloroform |% ? acetyl bromide acetoneWhat does it mean forward or backward and does the k=5.0×10^23 even play a role in this
- Chemistry The total volume (in cm3) of an aqueous solution containing 1 kg of water and n moles of NaCl can be represented by the equationV = 1002.94 + 11.4822 n + 1.7128 n3 + 0.002715 n5/2Calculate the partial molar volume of NaCl for a solution containing 1.000 mol of NaCl. The partial molar volume of NaCl is _________ cm3/mol.1. Given the following mixture of two compounds 45.00 g of X (MW =78.00 g/mol)(density 1.128 g/mL) and 610.00 mL of Y (62.00 g/mol))(density 0.872 g/mL), calculate the mole fraction of X. 2. Given the following mixture of two compounds 25.00 mL of X (MW =87.00 g/mol)(density 1.077 g/mL) and 620.00 mL of Y (90.00 g/mol))(density 1.229 g/mL). The boiling point of pure Y is -3.00 degrees C. The molal boiling constant is 3.276 degrees C/m. What is the boiling point of the solution. 3. Given the following mixture of two compounds 35.00 mL of X (MW =75.00 g/mol)(density 0.879 g/mL) and 765.00 mL of Y (74.00 g/mol))(density 1.161 g/mL). The vapor pressure of pure Y is 24.00. Calculate the vapor pressure of the solution. 4. 3.82 grams of a water soluble ionic compound with the formula of A1X4 (Molar mass of 125.00 grams/mol) is dissolved in 64 grams of water. Calculate the expected boiling point of the solution. The boiling point elevation constant for water is 0.512 degrees C/molal. The…(10) You have 4 powdered samples, A, B, C, & D. One sample contains fullerenes, C16 to C70. Another is nano diamond. Another one is a mixture of C60 and carbon nanotubes. The 4th is a mixture of graphite & graphene. Indicate the analytical methods you would use to identify and distinguish the samples from each other.