Lab 8 A student prepared a stock solution by dissolving 10.0 g of KOH in enough water to make 150. mL of solution, She then took 15.0 mL of the stock solution and diluted it with enough water tomake water to make 65.0 mL of a final solution. What is the concentration of KOH for the final solution?For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac).A v*G 哈QВIParagraphArial10ptABC v田田田EXO WORDS POWERED BY TINY

We have to determine concentration of final solution of KOH.

Answered: A student prepared a stock solution by…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 120QRT

See similar textbooks

Similar questions

We can measure the concentration of HCl solution by reaction with pure sodium carbonate:Complete reaction with 0.9674 ± 0.0009 g of Na2CO3 (FM 105.9884 ± 0.0007) required 27.35 ± 0.04mL of HCl. Find the molarity of the HCl and its relative and absolute uncertainties. Report themolarity to the correct number of digits. What is the major source of uncertainty in the molarity?
You 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.
In the Analytical Chemistry laboratory, one of the B.Sc student Ms. Fatma wanted to analyze the presence of Iron(II) ion in the water samples collected from Sohar Industrial Area in the Sultanate of Oman and analyzed by Spectrophotometric method. (1) 250.00 mL of this water sample (Solution A) known to contain unknown amount of FeSO4. She has diluted Solution A by a dilution factor 10 to make 250.00 mL solution, which she labeled Solution B. Using Spectrophotometer, she has measured the absorbance value (0.642) for Solution B at 508 nm using 1.00 cm cell (cuvet). The molar absorptivity value for Fe2* ion at 508 nm is ɛ508 = 30.8 M-1cm1. (i) What volume of the solution A did she require to make the 250.00 mL of Solution В? (ii) in (i)? What instrument should she use to transfer the volume of the Solution A calculated (ii) Concentration of FeSO4 in Solution B. (iv) Concentration of FeSO4 in Solution A. Mass of FeSO4 in Solution A (Show your calculation) (v)
The toxicity of DDT (C14H9Cl5) led to a ban on its use in the United States in 1972. Determinations of DDT concentrations in groundwater samples from Pennsylvania between 1969 and 1971 yielded the following results: Location Sample Size Mass of DDT Orchard 253 mL 0.0310 mg Residential 1.77 L 0.0350 mg Residentialafter a storm 51.5 mL 0.570 mg Express these concentrations in millimoles per liter. Orchard= ___mmol/l Residental=___ mmol/l Residential after a storm=___ mmol/L
A student creates a calibration plot for serial dilutions of Cu(NO3)2. A graph of concentration in M (x-axis) versus absorbance (y-axis) gives a linear trendline of y = 0.345x - 0.11. e.) Copper(II) nitrate has a solubility of 83.5 g in 100 g of water. Calculate the percent error in the student's concentration.
Beaker 0.00200 M Fe(NO3)3, mL 0.00200 M NaSCN, mL total volume, mL 1 3.000 2.000 10.00 2 3.000 3.000 10.00 3 3.000 4.000 10.00 4 3.000 5.000 10.00 5 (blank) 3.000 0.000 10.00 In Solutions 1-4 you are adding successively larger volumes of 0.00200M SCN- to the Fe3+ solution and diluting to 10.00 ml. Calculate the final diluted molarity of SCN- in solution #1 Your answer should have 3 sig figs =
Exactly 10.00-mL aliquots of a solution containing phenobarbital were measured into 50.00-mL volumetric flasks and made basic with KOH. The following volumes of a standard solution of phenobarbital containing 2.000μg/mL of phenobarbital were then introduced into each flask and the mixture was diluted to volume: 0.000, 0.500, 1.00, 1.50, 2.00 mL. The fluorescence of each of these solutions was measured with a fluorimeter, which gave values of 3.26, 4.80, 6.41, 8.02, 9.56, respectively. a. plot the data. b. derive a least squares equation for the data plotted in (a). c. find the concentration of phenobarbital from the equation in (b). d. calculate a standard deviation for the concentration obtained in (c).
You want to make a solution of the primary standard sodium oxalate. It has a molecular mass of 133.999 g/mol (no error). Your analytical balance has an error of 0.2 mg. You add some weighing paper to the balance and it reads a mass of 0.23626 g. You then add sodium oxalate onto the weighing paper until the mass registers as 2.8539 g. You carefully transfer this to a 250.0 ml volumetric flask with an error of 0.1 ml and dissolve the sodium oxalate in a sufficient volume of water. What is the concentration of the oxalic acid (in M) and what is the absolute error (also in M).
8 = filled CHM-202 Lab 1 Solids and Solutions Rev 1 G6-2022 Results: 1. Models of Crystalline Unit Cells Atomic Radius (radius of styrofoam ball) Volume of one atom (one ball, 4/3r¹) Measured unit cell length (1) [1.3] No. Atoms per cell [1.3] Ratio of 1/r [1.3] Geometric unit cell length (1) [1.5a] Volume of atoms in cell [1.5c] Total 3 Volume of Unit Cell [1.5c] Percent vol filled [1.5d] Percent free space. [1.5d] I atom Simple Cubic SC 6.15mm 118 6.9 172 Raw Data (Temperature vs. Time) Trial Time CHM-202 Lab 2 Freering Point Depression Rev2 06-2022 232.6 Temp Time d= 6.9 r = 3.24 Sum v=172²³² Body Centered Cubic BCC 8 lan a atom 2.3 7.96 344 531.45 B. Cyclohexane Solutions (Trial 4 if needed) Temp Time (include units!) (include units!) Face Centered Cubic FCC (CCP) 10.8cm 4 atom 7/12 3.13 Temp 5.26 688 1259-73 Time the pieces are not Temp
When drinking water is disinfected with chlorine, an undesired byproduct, chloroform (CHCl3), may form. Suppose a 70-kg person drinks 2 L of water every day for 70 years with a chloroform concentration of 0.08 mg/L (the drinking water standard). Potency factor for chloroform = 6.1 x 10-3 (mg/kg-day)-1 The upper-bound cancer risk for this individual. a. 0.545 b. 5.45x10-6 c. 5.45x10-4 d. 5.45x10-10 e. 14x10-6 If a city with 300,000 people in it also drinks the same amount water described in the above question, how many extra cancers per year would be expected? Assume the standard 70-year lifetime. a. 0.163 b. 1.63x10-4 c. 1.63x10-3 d. 1.63x10-6 e. 6x10-2
Calculate the molarity of a NaCI solution prepared by mixing 75.0 mL of a 6.0 M NaCl solution with enough water so that the final volume of the solution is 500.0 mL. For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac).
Exactly 1.00 grams of granular table salt was dissolved in deionized water up to 500 mL. An aliquot of 20 mL was titrated with AgNO3 (T = 8244 mg/mL) and consumed 46.60 mL to reach end point. If the impurities are just water, calculate the percent Moisture. Ans in 1 sig figure.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS