Q: 4. What volume of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.274 M NazS04…
A: Since you have posted multiple questions, we are entitled to answer the first only. 4) Given:…
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A: First calculate mole of each substance by dividing molar mass to the mass then calculate mole of…
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A: Molarity of a NaCl solution is equal to the number of moles of NaCl dissolved in one liter of a…
Q: 4.81 If 30.0 mL of 0.150 M CaCl2 is added to 15.0 mL of0.100 M AgNO3, what is the mass in grams of…
A: Solution : Stoichiometry in Chemistry is used to understand the relationship between reactants and…
Q: A bottle is labeled 0.26 M KMNO4. The KMNO4 will be used in the same reaction as took place in this…
A: Since you have posted multiple questions, we are entitled to answer the first only.
Q: What volume of 0.205 M K3PO4 solution is necessary to completely react with 142 mL of 0.0112 M NiCl2…
A: Molarity = number of moles of solute/volume of solution (in L) so, number of moles = molarity ×…
Q: What volume in mL of 0.220 M HBr solution is required to produce 0.0125 moles of HBr?
A: Given : Concentration of HBr = 0.220 M And moles of HBr = 0.0125 mol
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A:
Q: 780 mL of 0.0160 M AgNO, from the solid reagent. mL. Dissolve g AgNO, in enough water to give a…
A: a.) To calculate the grams of AgNO3 needed ,we would use Molarity formula . (Note : Please upload…
Q: If 33.4 g of CH3OH (MM = 32.04 g/mol) are dissolved in 500.0 mL of solution, what is the…
A: Given, amount of CH3OH =33.4 gMolar mass of CH3OH =32.04 g/molVolume of solution =500.0 mL =0.5 Lwe…
Q: What concentration of Br results when 847 mL of 0.403 M KBr is mixed with 961 mL of 0.447 M FeBr, ?…
A: Molarity of KBr is 0.403 M. Volume of KBr is 847 mL. Molarity of FeBr2 is 0.447 M. Volume of FeBr2…
Q: What volume of a 0.100 m heck is required to react with 2.35 g of sodium carbonate? Write the…
A: Balanced equation of HCl and sodium carbonate (Na2CO3 ) Na2CO3 + 2 HCl = 2 NaCl + H2O + CO2 Ionic…
Q: What volume in mL of 0.220 M HBr solution is required to produce 0.0175 moles of HBr?
A: MOLES= VOLUME (L) * MOLARITY
Q: what mass of iron (III) hydroxide percipitate can be produced by reacting 86.0 mL of 0.110M iron…
A: Reaction is given below:
Q: What mass of Naz CrO4 is required to precipitate all of the silver ions from 45.0 mL of a 0.600 M…
A: Given : Concentration of AgNO3 = 0.600 M Volume of AgNO3 solution = 45.0 mL = 0.045 L…
Q: Barium can be analyzed by precipitating it as Bas04 and sample of a barium compound was treated with…
A: In the given reaction Barium compound is treated with excess of sulphuric acid. In the given…
Q: 16. What is the molarity of the solution formed by mixing 0.20 mol of sodium hydroxide with enough…
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Q: Consider the following precipitation reaction: 2Na3PO4(aq) + 3CuCl2(aq)➡️Cu3(PO4)2(s) + 6NaCl(aq)…
A: Molarity of a solution is defined as the number of moles of solute present in one litre of a…
Q: 2) What volume of a 0.0225 M solution of potassium permanganate are required to titrate 0.461 g of…
A:
Q: If 41.5 g of CH₃OH (MM = 32.04 g/mol) are dissolved in 500.0 mL of solution, what is the…
A: The molarity of the solution is defined by the mole of solute present in one liter of solution. The…
Q: A bottle is labeled 0.26 M KMNO4. The KMNO4 will be used in the same reaction a. took place in this…
A: In this question, we want to determine the volume of the Solution, approximately, must be used to…
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A: Given: Volume of barium chloride is 0.4 L Molarity of barium chloride is 0.236 M Volume of Na3PO4 is…
Q: 5. How many grams of lead(II) iodide will precipitate when 45.0 mL of 0.500 M lead(II) nitrate…
A: Reaction is : Pb(NO3)2(aq) + 2KI(aq)-> PbI2(s) + 2KNO3(aq) Precipitated product is PbI2(s)…
Q: he chloride ion concentration in a solution may be determined by the precipitation of silver…
A: Given that, M1=0.7350 MV1=19.22 mLM2=?V2=25 ml
Q: How many grams of KNO3 (molar mass = 101.103 g/mol) should be used to make 170.0 mL of 0.060 M…
A: The values are given as follows:
Q: One liter of a solution is prepared by dissolving 125.6 g of NaF in it. If I took 180. mL of that…
A: Number of moles=Given massMolar mass
Q: What mass of Na2 CrO4 is required to precipitate all of the silver ions from 25.0 mL of a 0.200 M…
A: Molarity of AgNO3 = 0.200 M Volume of AgNO3 solution = 25.0 mL = (25.0 / 1000 ) L = 0.025 L We need…
Q: If 45.6 g of CH₃OH (MM = 32.04 g/mol) are dissolved in 500.0 mL of solution, what is the…
A: Given, 45.6 g of CH₃OH (MM = 32.04 g/mol) are dissolved in 500.0 mL of solution
Q: How many milliliters of a 0.200 M potassium chloride solution should be added to 34.0 mL of a 0.430…
A:
Q: A solution of 100.0 mL of 0.200 M KOH is mixed with a solutionof 200.0 mL of 0.150 M NiSO4. (a)…
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Q: A) If 500 mL of .300 M silver nitrate are mixed with 200mL of 0.5 M calcium chloride, how many grams…
A: In a balanced equation, the number of atoms on both sides of the equation should be identical. The…
Q: . Suppose 0.400 L of a solution of 0.0700 M nitric acid is added to 0.800 L of a solution of 0.0300…
A: Given : Concentration of Nitric acid i.e HNO3 in solution 1 = 0.0700 M Volume of solution 1 = 0.400…
Q: 61. What mass of Na2 CrO4 is required to precipitate all of the silver ions from 75.0 mL of a…
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Q: One liter of a solution is prepared by dissolving 157.6 g of NaF in it. If I took 80. mL of that…
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Q: Solution X containing 0.020 mol of iron(II) sulfate requires 22.5 mL of potassium manganate(VII) for…
A: Given, The number of moles (n)= 0.020 mol The volume of KMnO4 (V)=22.5 mL=0.0225 L
Q: 98. Calculate the volume in milliliters of 0.563 M barium hydroxide solution required to precipitate…
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A:
Q: What volume in mL of 0.220 M HBr solution is required to produce 0.0210 moles of HBr?
A: Number of moles = Molarity (mol/L ) × Volume( L)
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A: Answer: The concentration of the resulting solution is 0.158 mol/L.
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A: Given, Molar mass of ammonium carbonate = 96.09 g/mol Volume of ammonium nitrate = 358 mL Molarity…
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A: Given data for part (a) stock solution Molarity (M1) =14.8 M Final solution Molarity (M2) = 0.250 M…
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A: Given, Volume of LiCl = 859 mL Concentration of LiCl = 0.519 M Volume of MgCl2 = 675 mL…
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Q: If 13.00 mL of 0.6920 M barium chloride are reacted with 16.00 mL of 0.8690 M silver nitrate, how…
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Q: Suppose 60.0 mL of 0.100 M Pb(NO3)2 is added to 30.0 mL of O.150 M KI. How many grams of Pbl, will…
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Q: Solution X containing 0.020 mol of iron(II) sulfate requires 22.5 mL of potassium manganate(VII) for…
A: Given: The number of moles (n) is 0.020 mol. The volume of KMnO4 (V) is 22.5 mL. To find: Molarity…
Q: What mass (in g) of silver chloride (MM = 142.32 g/mol) is formed from the reaction of 157.4 mL of a…
A: Molarity (M) :- The number of moles of solute dissolved in 1 litre of solution is defined as…
Q: Suppose 30.0 mL of 0.100 M Pb(NO3) is added to 60.0 mL of 0.150 M KI. How many grams of Pbl2 will be…
A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…
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- A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.400 M HCl. The solution was then treated with an excess of aqueous chromium(III) nitrate, resulting in formation of 2.06 g of precipitate. Determine the concentration of the NaOH solution.Relative solubilities of salts in liquid ammonia can differsignificantly from those in water. Thus, silver bromide issoluble in ammonia, but barium bromide is not (thereverse of the situation in water). Write a balanced equation for the reaction of anammonia solution of barium nitrate with an ammoniasolution of silver bromide. Silver nitrate is soluble inliquid ammonia. What volume of a 0.50 M solution of silver bromidewill react completely with 0.215 L of a 0.076 M solutionof barium nitrate in ammonia? What mass of barium bromide will precipitate fromthe reaction in part (b)?A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00102M HCl requires 36.6 mL of the acid to reach the end point. Ca(OH)2(aq)+2HCl(aq)CaCl2(aq)+2H2O(l) What is the molarity?
- What mass of solid AgBr is produced when 100.0 mL of 0.150 M AgNO3 is added to 20.0 mL of 1.00 M NaBr?A 50.00-mL sample of 0.0250 M silver nitrate is mixed with 0.0400 M chromium(III) chloride. (a) What is the minimum volume of chromium(III) chloride required to completely precipitate silver chloride? (b) How many grams of silver chloride are produced from (a)?Twenty-five milliliters of a solution (d=1.107g/mL)containing 15.25% by mass of sulfuric acid is added to 50.0 mL of 2.45 M barium chloride. (a) What is the expected precipitate? (b) How many grams of precipitate are obtained? (c) What is the chloride concentration after precipitation is complete?
- What mass of solid aluminum hydroxide can be produced when 50.0 mL of 0.200 M Al(NO3)3 is added to 200.0 mL of 0.100 M KOH?Iron (II) can be oxidized to iron (III) by dichromate ion, which is reduced to chromium (III) in acid solution. A 2.5000-g sample of iron ore is dissolved and the iron converted into iron(II). Exactly 19.17? ml. of 0.0100 M Na2Cr2O7 is required in the titration. What percentage of the ore sample was iron?A 100.0-mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0 mL of 0.200 M aqueous magnesium nitrate. a. Write a balanced chemical equation for any reaction that occurs. b. What precipitate forms? c. What mass of precipitate is produced? d. Calculate the concentration of each ion remaining in solution after precipitation is complete.
- 68. Aluminum ion may be precipitated from aqueous solution by addition of hydroxide ion, forming Al(OH)3. A large excess of hydroxide ion must not be added, however, because the precipitate of Al(OH)3 will redissolve as a soluble compound containing aluminum ions and hydroxide ions begins to form. How many grains of solid NaOH should be added to 10.0 mL of 0.250 M A1Cl3 to just precipitate all the aluminum?A solution contains both iron(II) and iron(III) ions. A sample Of the solution is titrated with 35.0 ml, of M KMnO4, which oxidizes Fe2+ to Fe3+. The permanganate ion is reduced to manganese(ll) ion. The equation for this reaction is MnO4(aq)+8 H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+ +4H2OAnother 50.00-mL sample of the solution is treated with zinc, which reduces all the Fe3+ to Fe2+. The equation for this reaction is 2Fe3+(aq)+Zn(s)2Fe2+(aq)+Zn2+(aq)The resulting solution is again titrated with 0.0280 M KMnO4; this time 48.0 ml, is required. What are the concentrations of Fe2+ and Fe3+ in the solution?What mass of silver chloride can be prepared by the reaction of 100.0 mL of 0.20 M silver nitrate with 100.0 mL of 0.15 M calcium chloride? Calculate the concentrations of each ion remaining in solution after precipitation is complete.