A 40.0-ml solution contains 0.021 M barium chloride (BaCl2). What is the minimum concentration of sodium...
A 40.0-mL solution contains 0.033 M barium chloride (BaCl2). What is the minimum concentration of sodium sulfate (Na2SO4) required in the solution to produce a barium sulfate (BaSO4) precipitate? The solubility product for barium sulfate is Ksp = 1.1 ✕ 10−10.
a)A solution of saturated PbBr2 is found to contain 2.4 ✕ 10−2M bromide ion. Calculate the Ksp of PbBr2. b) A 40.0-mL solution contains 0.029 M barium chloride (BaCl2). What is the minimum concentration of sodium sulfate (Na2SO4) required in the solution to produce a barium sulfate (BaSO4) precipitate? The solubility product for barium sulfate is Ksp = 1.1 ✕ 10−10. c)The solubility product, Ksp, for magnesium hydroxide, Mg(OH)2, is 5.6 ✕ 10−12 at 25°C. What is the molar solubility...
Sodium sulfate, Na2SO4, and barium chloride, BaCl2, are soluble compounds that form clear solutions. However, when aqueous solutions of sodium sulfate and barium chloride are mixed together, a white solid (a precipitate) forms as shown in the image below. 10 Question (3points) a See page 170 Sodium sulfate, Na2SO4, and barium chloride, BaCl2, are soluble compounds that form clear solutions. However, when aqueous solutions of sodium sulfate and barium chloride are mixed together, a white solid (a precipitate) forms as...
Barium chloride and sodium sulfate react according to the following equation. BaCl2 + Na2SO4 → BaSO4 + 2Naci Answer the question(s) that follow about this reaction. How many grams of barium sulfate can be produced from 74.8 g of barium chloride?
(7. Consider the reaction as follows: Na2SO4(aq) + BaCl2(aq) → BaSO4(s) + 2 NaCl(aq) A 1.00-mol sample of sodium sulfate was placed into the barium chloride aqueous solution to make solid barium sulfate. (a) How many gram of sodium sulfate was placed into the reaction solution? (b) What is the maximum mass of NaCl formed? (c) If 78.9 g of NaCl was obtained, what was the percent yield of NaCl? 3. How many liters of 0.186 M of NaOH (aq)...
7. A 25.0 mL solution of 0.0015M BaCl2 is added to 20.0 mLs of 0.0010 M Na2SO4. Determine if the resulting solution will have a precipitate form or if it will remain unsaturated. Ksp (BaSO4) = 1.1.x 10-10
A solution contains 0.040 M of Na2SO4 and 0.050 M of NaIO3. Another solution of Ba2+ is added to the first solution.( You must accept that the original solution does not include HSO-4). a) Which of the Baryum salts precipitate firstly? b) Calculate the Ba2+ concentration while the first precipitate is occuring. c) While the more dissolved precipitate is precipitating, what is the concentration of anion which forms the less dissolved Baryum salt ? Ba(IO3) Ksp= 1.57x10-9 BaSO4 Ksp= 1.1x10-10
A) A buffer solution contains 0.10 mol of acetic acid and 0.13 mol of sodium acetate in 1.00 L. What is the pH of the buffer after the addition of 3×10−2 mol of HNO3? Express your answer using two significant figures. C) Barium sulfate, BaSO4, is used in medical imaging of the gastrointestinal tract because it is opaque to X rays. A barium sulfate solution, sometimes called a cocktail, is ingested by the patient, whose stomach and intestines can then...
An aqueous solution of sodium fluoride is slowly added to a water sample that contains barium ion (4.65x10-2 M) and calcium ion (7.40x10-2 M).The Ksp of barium fluoride is 1.00x10-6. The Ksp of calcium fluoride is 3.90x10-11. What is the remaining concentration of the first ion to precipitate when the second ion begins to precipitate?
Purifying Mg2+ from sea water. Aqueous sodium hydroxide is added to an aqueous solution that contains 0.0099 M magnesium chloride and 0.021 M calcium chloride. What will be the concentration of the metal ion that precipitates first (as M(OH)2) at the time the second metal ion begins to precipitate? Ksp (Mg(OH)2) = 6.3 x 10-10 and Ksp (Ca(OH)2) = 6.5 x 10-6 Hint: Use Ksp values to determine the solubility of each product to determine the order of precipitation.