If you dissolve 20.000 g of KSCN(s) in a 250.00 mL volumetric flask, and fill the flas exactly to the mark, what is the concentration of KSCN you have prepared? a. 8.2321 x 103 M b. 0.82321 M
Q: 645 grams of pond water sample were gathered and known to contain 1.45 x 10 grams of cadmium. What…
A: ppb is stand for part per billion and is a way of expressing concentration of solution.
Q: A) What is the mass in grams of 1.59 moles of aluminum oxide? (a) 64.1 g…
A: Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: Concentrated sulfuric acid, H2SO4, is about 18 M. If 75 mL of this solution is diluted to 1.5 L and…
A: In the given problem, the molarity of the serially diluted solution can be calculated by using the…
Q: Toxic Cr(VI) can be precipitated from an aqueous solution by bubbling SO2 through the solution. How…
A: Given;
Q: Can you please help me with this problem?
A: Calculate the number of moles of HCl.
Q: 4. Given a stock 14.8 M ammonia solution a. How many milliliters of this solution must you dilute to…
A: Number of moles of ammonia = Concentration of ammonia (M) × Volume of solution (L) Number of moles…
Q: In the laboratory, a student adds 21.7 g of manganese(II) chloride to a 125 mL volumetric flask and…
A: Given : Mass of MnCl2 i.e Manganese (II) chloride = 21.7 g And volume of solution = 125 mL = 0.125 L…
Q: Use the graph to the right to answer the next three questions: Solubility Curves 150 12. If 100 g of…
A: Answer:- This question is answered by using the simple concept of solubility and using the given…
Q: What volume (mL) is required from a stock solution of1.98 M KNOg to prepare a 750 mt solution of…
A: Given that: Molarity of stock KNO3 solution(M1) = 1.98M Molarity of final KNO3 solution(M2) = 1.00M…
Q: 5. How many grams of potassium sulfate would be recovered by evaporating 623 mL of 22.5 % potassium…
A: Mass = Volume x density %Mass = 100 x Mass of solute/Mass of solution Number of moles = Molarity x…
Q: A solution is prepared by dissolving 2.86 g KMnO4 in 75.0 mL of water. (Density H₂O = 1.00 g/mL).…
A: Mass percent is calculated using the mass of solute and total mass of solution .
Q: 29. How many grams of Al(OH)3 can be produced from 100 mL of 0.300 M Ba(OH)2?…
A: The given reaction is, 3 Ba(OH)2 + 2 AlCl3 -----> 2 Al(OH)3 + 3 BaCl2 Given,…
Q: What volume (mL) is required from a stock solution of 1.98 M KNO3 to prepare a 750 mL solution of…
A:
Q: An experiment calls for 211 mL of 0.401 MNaCl solution. What mass of NaCl is required? Mass = What…
A:
Q: (a) How many milliliters of a stock solution of 13.0 M HNO3 would you have to use to prepare 0.500 L…
A:
Q: please highlight the correct answer
A: The expression for dilution (d) in terms of the ratio of volumes is determined as follows:
Q: A student makes a solution by dissolving 4.875 g of K2CO3 (MM = 138.205 g/mol) in 200.0 mL of water.…
A: Molarity is defined as “the mole of the solute per unit volume of the solution”. It is represented…
Q: How many milliliters of a 0.223 M Rb NO 3 solution contain 0.250 moles of Rb NO 3 ? 1.12 × 103 mL…
A: Data: Molarity of RbNO3 solution = 0.223 M Moles of RbNO3 = 0.250 moles To find volume of solution…
Q: A solution of bromine in dichloromethane contains 5.0 % bromine by volume. The density of pure,…
A:
Q: After the complete evaporation of water in a saltwater, there are 0.505 g of NaCl left in the…
A: In this question, we will calculate the Molarity ( Concentration ) of NaCl in original Solution.…
Q: 35. How many grams of ammonium chloride (molar mass = 53.5g/mol) are contained in 0.500 L of a 2.00…
A:
Q: 13.58 An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d = 1.114…
A:
Q: 3. Dilution: Determine the concentration of a solution prepared by diluting 25.0 mL of a stock 0.188…
A: Given Molarity of Ca(NO3)2 ( M1) = 0.188 M Volume of stock solution ( V1 ) = 25 mL Final…
Q: A solution is made by dissolving 17.8 g of magnesium sulfite, MGSO3, in enough water to make exactly…
A:
Q: Suppose you need to prepare 1.00 L of 0.100 M HCl(aq), and all you have on hand is 0.250 M HCl(aq).…
A: The given question is from dilution of HCl. During dilution no. Of moles do not changes. So, M1V1=…
Q: Zinc dissolves in hydrochloric acid to yield hydrogen gas: Zn(s) + 2HCI(aq) → ZnCl2(aq) + H2(g) What…
A: Using stoichiometric ratio we can determine how many moles of each reactant reacts . From that we…
Q: A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. If the density of the…
A:
Q: A solution is made by dissolving 17.8 g of magnesium sulfite, MgSO3, in enough water to make exactly…
A: Molarity is defined as number moles of solute in 1 litre of solution.
Q: A solution is made by dissolving 17.8 g of magnesium sulfite, MgS03, in enough water to make exactly…
A: Molarity can be defined as the ratio of number of moles of solute to volume of solution in liter(L).…
Q: What is the mass in grams of potassium dichromate(K2Cr207) are required to prepare a 350 cm3…
A:
Q: What is the mass in grams of potassium dichromate(K,Cr,0,) are required to prepare a 350 cm?…
A: Option B) 531g
Q: AGNO3 solutions are often used to plate silver onto other metals. What is the maximum amount of…
A: The number of moles is a ratio of the mass of a substance to the molar mass of the substance.…
Q: What volume of a 0.43 M ZnCl2 solution contains 2.52 g of ZnCl2? Mw ZnCl2 = 136.29 g/mol. %3D OA…
A: We know that Molarity = number of moles of solute / volume of the solution in L Number of moles =…
Q: A man’s blood has lead levels of 80. micrograms/ 100.0 mL. 5.0 mL of 2.0 M Na2Ca(EDTA) is…
A: Given:- Volume of Na2Ca(EDTA) V = 5.0 mL x (1L/1000 mL)…
Q: Consider a rxn in which Mg metal reacts with Hcl to form aqueous magnesium chloride and hydrogen…
A: We have to calculate the mass of hydrogen gas produced .
Q: Calculate the volume (in L) of a solution that contains 3.12 moles of NaCl if the concentration of…
A: number of moles of NaCl = 3.12 moles Molarity = 6.67 M
Q: 1. 1. What is the difference between dilution and concentration? B iUFont Family - AA A E E E - @ 因…
A: Dilution : Dilution refers to the process of adding additional solvent to a solution to decrease its…
Q: A solution was prepared by dissolving 2.85 g of MgCh in sufficient water to give 3.000 L. Calculate…
A: Given: Weight of MgCl2 = 2.85 g Volume of water = 3 L Volume of Cl- ions = 50 mL = 0.05 L Atomic…
Q: A 1.00 mL sample of seawater is determined to contain 2.50 × 10-14 moles of dissolved gold. How…
A:
Q: Determine the concentration of a solution prepared by diluting 25.0 mL of a stock 0.188 M Mg(NO3)2…
A:
Q: water and heated. The solution is then cooled. How many grams of the impurity will crystallize when…
A: In the given question we have to calculate the grams of impurity will crystallize when the solution…
Q: 1) What is the concentration in ppm of a solution made with 18.5 g of salt and 125000.00 g of water?…
A:
Q: Nitric acid is a potentially dangerous strong acid that must be handled with great care. A…
A:
Q: The concentration of solution A is 2.0 mol / dm3. Prepare solution B as follows: Pipette solution A…
A: We can solve for the concentration or volume of the concentrated or dilute solution using the…
Q: 1. A 0.1430 g sample of copper was dissolved in 20 mL of 6 mol/L HNO3 and diluted to 100.0 mL in a…
A: The concentration of the standard solution in terms of g/L is 0.0143 g/L. Since the intercept on the…
Q: A solution is prepared by dissolving 52.3 g of RÜC1 in enough water to form 502 mL of solution.…
A: Consider the given information is as follows; Mass of RbCl = 52.3 g Volume of solution = 502 mL…
Q: What is the volume of a solution that contains 18.2 grams HCl (molar mass = 36.46 g/mol) in a 0.750…
A:
Q: What is the mass in grams of potassium dichromate(K2Cr207) are required to prepare a 350 cm3…
A: Moles = Molarity × Volume (L) Moles = 5.16 × 350/1000 Moles = 1.806 ( 1L = 1000 cm^3 )
Q: What is the concentration of a diluted solution of magnesium chlorite? The concentrated stock had a…
A: Initial concentration (stock solution), M1 = 1.40 M The initial volume, V1 =50.0 mL= 0.050 L Final…
Step by step
Solved in 2 steps with 3 images
- In most of its ionic compounds, cobalt is either Co(II) or Co(III). One such compound, containing chloride ion and waters of hydration, was analyzed, and the following results were obtained. A 0.256-g sample of the compound was dissolved in water, and excess silver nitrate was added. The silver chloride was filtered, dried, and weighed, and it bad a mass of 0.308 g. A second sample of 0.416 g of the compound was dissolved in water, and an excess of sodium hydroxide was added. The hydroxide salt was filtered and heated in a flame, forming cobalt(III) oxide. The mass of cobalt(III) oxide formed was 0.145 g. a. What is the percent composition, by mass, of the compound? b. Assuming the compound contains one cobalt ion per formula unit, what is the formula? c. Write balanced equations for the three reactions described.You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g. a. If you had an extremely magnified view of the solution (to the atomic-molecular level), list the species you would see (include charges, if any). b. Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges. c. Calculate the percent sodium chloride in the original unknown mixture.Consider an experiment in which two burets, Y and Z, are simultaneously draining into a beaker that initially contained 275.0 mL of 0.300 M HCl. Buret Y contains 0.150 M NaOH and buret Z contains 0.250 M KOH. The stoichiometric point in the titration is reached 60.65 minutes after Y and Z were started simultaneously. The total volume in the beaker at the stoichiometric point is 655 mL. Calculate the flow rates of burets Y and Z. Assume the flow rates remain constant during the experiment.
- Sulfuric acid is listed in a catalog with a concentration of 95-98%. A bottle of the acid in the stockroom states that 1.00 L has a mass of 1.84 kg. To determine the concentration of sulfuric acid in the stockroom bottle, a student dilutes 5.00 mL to 500. mL She then takes four 10.00-mL samples and titrates each with standardized sodium hydroxide (c = 0.1760 M). (a) What is the average concentration of the diluted sulfuric acid sample? (b) What is the mass percent of H2SO4 in the original bottle of the acid?Using the general solubility rules discussed in Chapter 7, give the formulas of live substances that would be expected to be readily soluble in water and five substances that would be expected to not be very soluble in water. For each of the substances you choose, indicate the specific solubility rule you applied to make your prediction.In the spectroscopic analysis of many substances, a series of standard solutions of known concentration are measured to generate a calibration curve. How would you prepare standard solutions containing 10.0, 25.0, 50.0, 75.0, and 100. ppm of copper from a commercially produced 1000.0-ppm solution? Assume each solution has a final volume of 100.0 mL. (See Exercise 123 for definitions.)
- Apply Students conducted a lab to investigate limiting and excess reactants. The students added different volumes of sodium phosphate solution (Na3PO4) to a beaker. They then added a constant volume of cobalt(ll) nitrate solution (CO(NO3)2) stirred the contents, and allowed the beakers to sit overnight. The next day, each beaker had a purple precipitate at the bottom. The students decanted the supernatant from each beaker, divided it into two samples, and added one drop Of sodium phosphate solution to one sample and one drop of cobalt(ll) nitrate solution to the second sample. Their results are shown in Table 11.5. a. Write a balanced chemical equation for the reaction. b. Based on the results, identify the limiting reactant and the excess reactant for each trial.A 2.5624-g sample of a pure solid alkali metal chloride is dissolved in water and treated with excess silver nitrate. The resulting precipitate, filtered and dried, weighs 3.03707 g. What was the percent by mass of chloride ion in the original compound? What is the identity of the salt?It took 25.06 0.05 mL of a sodium hydroxide solution to titrate a 0.4016-g sample of KHP (see Exercise 79). Calculate the concentration and uncertainty in the concentration of the sodium hydroxide solution. (See Appendix 1.5.) Neglect any uncertainty in the mass.
- Oyster beds in the oceans require chloride ions for growth. The minimum concentration is 8 mg/L (8 parts per million). To analyze for the amount of chloride ion in a 50.0-mL sample of water, you add a few drops of aqueous potassium chromate and then titrate the sample with 25.60 mL of 0.001036 M silver nitrate. The silver nitrate reacts with chloride ion, and, when the ion is completely removed, the silver nitrate reacts with potassium chromate to give a red precipitate. (a) Write a balanced net ionic equation for the reaction of silver nitrate with chloride ions. (b) Write a complete balanced equation and a net ionic equation for the reaction of silver nitrate with potassium chromate, indicating whether each compound is water-soluble or not. (c) What is the concentration of chloride ions in the sample? Is it sufficient to promote oyster growth?The units of parts per million (ppm) and parts per billion (ppb) are commonly used by environmental chemists. In general, 1 ppm means 1 part of solute for every 106 parts of solution. Mathematically, by mass: ppm=gsolutegsolution=mgsolutekgsolution In the case of very dilute aqueous solutions, a concentration of 1.0 ppm is equal to 1.0 g of solute per 1.0 mL, which equals 1.0 g solution. Parts per billion is defined in a similar fashion. Calculate the molarity of each of the following aqueous solutions. a. 5.0 ppb Hg in H2O b. 1.0 ppb CHCl3 in H2O c. 10.0 ppm As in H2O d. 0.10 ppm DDT (C14H9Cl5) in H2OWhat volume of 0.0105-M HBr solution is required to titrate 125 mL of a 0.0100-M Ca(OH)2 solution? Ca(OH)2(aq)+2HBr(aq)CaBr2(aq)+2H2O(l)