Potassium nitrate was synthesized in an experiment using 10 mL of nitric acid and excess potassium hydroxide. The mass data obtained from the experiment is shown in Table 1 below. Given that the percentage yield of potassium nitrate was 88.3 %, calculate the concentration (% m/v) of the nitric acid used in the experiment. Table 1: Mass data for the synthesis of potassium nitrate from nitric acid and potassium hydroxide Mass of clock glass and crystallized potassium nitrate/ g 45.55 Mass of empty clock glass/ g 39.18

Potassium nitrate was synthesized in an experiment using 10 mL of nitric acid and excess potassium hydroxide. The mass data obtained from the experiment is shown in Table 1 below. Given that the percentage yield of potassium nitrate was 88.3 %, calculate the concentration (% m/v) of the nitric acid used in the experiment. Table 1: Mass data for the synthesis of potassium nitrate from nitric acid and potassium hydroxide Mass of clock glass and crystallized potassium nitrate/ g 45.55 Mass of empty clock glass/ g 39.18

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

This reaction is used to obtain iron from iron ore: Fe2O3(s) + 3 CO(g) —>2 Fe(s) + 3 CO2(g) The reaction of 185 g of Fe2O3 with 95.3 g of CO produces 87.4 g of Fe. Determine the limiting reactant, theoretical yield, and percent yield. (include solution map & steps)
Consider the following chemical reaction HCl (aq) + HgNO3 (aq) à Hg2Cl2 (s) + HNO3 (aq) If 20.0 grams of HCl is mixed with 30.0 grams of HgNO3 Determine the excess reactant The amount of the solid precipitate that was recovered equals to .................. grams , if the percentage yield from this reaction was determined to be 78.4%. Write the net ionic equation for the chemical reaction Determine the type of this chemical reaction
The reaction below takes place in water at room tempeture. Balance the reaction and write the correct state of matter for the substance. CaCI_2(aq) + (NH_4)_3PO_4 -> Ca_3(PO_4)_2 + NH_4CI
What is the formula (solve for x) for the original hydrated sample of copper (II) sulphate? You weigh a sample of CuSO4 · XH2O. After you heat the sample, you find that the mass of the anhydrous salt is 1.47g. What is the value of x? CONTEXT Mass of just anhydrous compound = mass of anhydrous compound rod mass of beaker and 108.34g - 106.87g = 1.47g %3D %3D = original compound mass - anhydrous compound mass = 3.00g - 1.47g = 1.53g Mass of just water
Based on this. What was the percentage by mass of water in the sample?
[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant. b) Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 64.7 grams Al according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) c) Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 201 grams Fe₂O₃ according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) d) Which of the following substances is the limiting reactant? e) What is the mass in grams of the excess Fe₂O₃ remaining after the partial reaction of 201 g Fe₂O₃ with 64.7 g Al? Give your answer to three significant figures.
When answering this problem, report the answer with the appropriate number of significant figures. Enter your answer USING scientific notation. When entering units, use proper abbreviated units with proper capitalization. In this experiment, a series of solutions are prepared by combining multiple components into a single container. One solution prepared contains 5.00 mL of 0.010 molar KI, 10.00 mL of 0.0010 molar Na2S2O3, 15.00 mL of water, 10.00 mL of 0.040 molar KBrO3, and 10.00 mL of 0.10 molar HCl. What is the concentration of iodide ions in this solution? Answer: ____x10______units
Here is a graph of the molarity of glucose (C6H₁2O6) in a reaction vessel during a certain chemical reaction. Use this graph to answer the questions in the table below. M 0.30- 0.25- 0.195 0.10- 0.05- 0 500 1000 1500 seconds 2000 2500 # 3000 X Œ 3
+ Chemistry 20 Midterm Equation Sheet (Click to open) Nitric acid is a potentially dangerous strong acid that must be handled with great care. A laboratory technician is asked to dilute a sufficient quantity of stock 15.4 mol/L nitric acid to produce 1.50 L of a 0.220 mol/L solution. Calculate the volume of concentrated nitric acid needed to prepare this diluted solution. XQ F1 BI E E F2 2 E E F3 % F4 F5 U S X₂ x² E F6 II Proctorio is sharing your screen. Ⓡ F7 = I Stop sharing DO LL F8 5 C H Hide + F9 ✓ C F10
A student prepares phosphorous acid by reacting solid phosphorous triiodide with waterPI₃(s) + 3 H₂O(l) → H₃PO₃(s) + 3 HI(g)The student needs to obtain 0.359 L of phosphorous acid (d=1.651g/mL). The procedure calls for a 43.3 % excess of water and a yield of 70.8%. How much phosphorous triiodide should be weighed out?
5 g of hydrated barium chloride is heated in a crucible until the mass of the sample no longer changes. The mass of the sample after heating is 4.26 g. Assume that the mass lost during the heating is solely due to the loss of water from the sample. What percentage of water was contained in the barium chloride hydrate?
You are a researcher working in a famous molecular biology lab. You will be doing a very important experiment tomorrow and need to get ready by preparing several solutions. One of the solutions you will need to make is a stock solution of 3M magnesium chloride. Since you will need to use this solution many times, you decide to make 350 mL of this solution. You take out your container of magnesium chloride solid and take it to the balance. How many grams would you weigh to make 300 ml of this 3M stock solution? Atomic weight of Mg = 24.31 Atomic weight of Cl = 35.45 Write your answer with two digits past the decimal point. (Important - Trailing zeroes count as digits - (e.g. 12.00 counts as two digits past the decimal point). The answer is ___________________________ grams 85.5 g is not the correct answer