If so, write the formula of the precipitate. Is a barium sulfate (BaSO4) precipitate expected to form when 50.0 mL of 0.0010 M BaCl2 solution is added to 50.0 mL of 0.00010 M Na2SO4? The Ksp for barium sulfate is 1.1 x 10^-10. Does a precipitate form when Pb(NO3)2 reacts with FeCl3? If the answer is yes, write the formula of the precipitate.Web
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The pathway of the sparingly soluble salt can be easily monitored by x-rays. Will barium sulfate precipitate if 10.0 mL of 0.0020 M Na 2 SO 4 is added to 100 mL of 3.2 × 10 −4 M BaCl 2? Recall that (ce{NaCl}) is highly soluble in water. Given: K sp and …Web
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The precipitation of barium sulfate from aqueous solutions of barium chloride and sodium sulfate was investigated experimentally in a continuous Y-Mixer to …Web
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Barium is a silvery-white metal that occurs in nature in many different forms called compounds. These compounds are solids and they do not burn well. Two forms of barium, barium sulfate and barium carbonate, are often found in nature as underground ore deposits. Barium is sometimes found naturally in drinking water and food. Because …Web
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Barium sulfate. In Meyler's Side Effects of Drugs (Sixteenth Edition), 2016. General information. Oral barium sulfate is theoretically non-toxic, but constipation and abdominal pain are not uncommon after barium meals or barium enemas [1].The main risk is that collections of barium will remain in the colon; they can persist for 6 weeks or longer in …Web
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Barium sulfate is a soft crystalline solid. It is a rhombic crystal. The pure salt is white but the color of the mineral "barite" can vary between red, yellow, gray or green, depending on impurities. Its density is 4.50 g/cm 3 and its refractive index is 1.64. It melts around 1580 °C but decomposes above 1600 °C.Web
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Using thermodynamics, especially equations based on the HKF-SRK modified model, this paper describes typical conditions for barium sulphate …Web
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Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2 (aq) and 0.0370 M Ag (aq). What will be the concentration of Ca2 (aq) when Ag2SO4 (s) begins to precipitate? Is a barium sulfate (BaSO4) precipitate expected to form when 50.0 mL of 0.0010 M BaCl2 solution is added to 50.0 mL of 0.00010 M Na2SO4?Web
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Solid barium sulfate is placed into a beaker to form a saturated solution of barium sulfate. The solution has a barium concentration of 1 x 10^{-5}M. What is KSP for barium sulfate? Which of the following solutions could be mixed together to form a precipitate of silver sulfide? A. AgNO_3 and Na_2S. B. AgNO_3 and Na_2SO_4. C. AgClO_4 and CS_2. D.Web
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The worst scenario for barium sulfate precipitation occurred at a mixing ratio of 40:60 formation and injection waters. This ratio was used in the jar, turbidity, …Web
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3.1 Effect of Chelating Agent (K4-EDTA). Figure 2 illustrates the solubility behavior of Barium sulfate (BaSO 4) in 15 wt% HCl and 15 wt% K4-EDTA solutions.BaSO 4 exhibits poor solubility in acidic solutions such as hydrochloric acid (HCl). When BaSO 4 is introduced to HCl, it tends to remain primarily as a solid precipitate (shown in Fig. 2A). …Web
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An excess of potassium sulfate was added to 50.0 mL of the solution, and 1.128 g of barium sulfate precipitate formed. Assume that the original solution was barium chlor; What is the solubility of barium sulfate in a solution containing 0.050 M sodium sulfate? The K_{SP} value for barium sulfate is 1.1 times 10^{-10}.Web
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Any treatment method that concentrates barium, as is the case with ion exchange softening, reverse osmosis, and distillation may cause precipitation. Barium sulfate will precipitate at concentrations of 2 ppm or greater. If the sulfate level in the raw water is greater than 2 ppm, barium sulfate precipitation is likely.Web
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Count the number of atoms of each element on each side of the equation and verify that all elements and electrons (if there are charges/ions) are balanced. Since there is an equal number of each element in the reactants and products of BaCl2 + Na2SO4 = BaSO4 + 2NaCl, the equation is balanced. Balance the reaction of BaCl2 + Na2SO4 = BaSO4 ...Web
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Barium is a white liquid used to coat the organs of the digestive system during an X-ray. This can help to provide a clearer picture of a person's organs and bones to help reaching a diagnosis.Web
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The available information on barium has been assessed with the intent of establishing a drinking water guideline and guideline technical document. This draft guideline technical document proposes a new maximum acceptable concentration (MAC) of 2.0 mg/L (2,000 µg/L) for barium in drinking water, based on kidney effects in male mice.Web
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Write the net ionic equation for the reaction of sodium sulfate and barium chloride. Assume that a precipitate is formed. Consider the reaction when aqueous solutions of barium nitrate and potassium hydroxide are combined. Write the net ionic equation (include s, aq, l, or g) Consider the reaction when aqueous solutionsWeb
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When sodium sulphate solution is added to barium chloride, a white precipitate is formed. Write the chemical name of precipitate obtained and type of chemical reaction involved in this process. View Solution. Q4. What can be inferred from the following equation?Web
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Barium sulfate scales once formed on the equipment surfaces are extremely difficult to remove. Typically mineral scaling in oil and gas production is controlled by two methods: 1. Use of inhibitors to prevent formation, and 2. Mechanical removal (scraping, sand blasting, chipping) or chemical removal (use of acids orWeb
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During the production of hydrocarbons from subterranean reservoirs, scaling with calcium carbonate and barium sulfate causes flux decline and dangerous problems in production facilities. This work is intended to study the effect of calcium ions on the precipitation of barium sulfate (barite); then, the effect of the formed barite on calcium …Web
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Barium sulfate comes as a powder to be mixed with water, a suspension (liquid), a paste, and a tablet. The powder and water mixture and the suspension may be taken by mouth or may be given as an enema (liquid that is instilled into the rectum), and the paste and tablet are taken by mouth. Barium sulfate is usually taken one or more times before ...Web
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Generally, compounds containing sulfate ($ce{SO_4^2-}$) compounds are soluble. (For essentially the same reason that sulfuric acid $ce{H2SO4}$ is a strong acid, if you're interested.) Well-known insoluble sulfate compounds are $ce{PbSO4, SrSO4, CaSO4}$, and $ce{BaSO4}$. Note that all of these cations have a somewhat high (+2) …Web
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Aluminum chloride is created when barium chloride interacts with aluminum sulphate to form barium sulphate precipitate. The reaction's unbalanced equation is; BaCl2 (aq) + Al2(SO4)3 (aq) → AlCl3 (aq) + BaSO4 (s) Barium chloride + Aluminium sulfate → Aluminium chloride + Barium sulfate.Web
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K sp for barium sulfate at 298 K is 1.1 x 10-10 mol 2 dm-6. In order for this equilibrium constant (the solubility product) to apply, solid barium sulfate must be present in a saturated solution of barium sulfate. ... If the concentrations are lowered enough, no precipitate can form. However, it is impossible to calculate a product greater than ...Web
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Sulphite $(ce{SO3^2-})$ and Barium Choride $(ce{ BaCl2})$ or Strontium Chloride $(ce{ SrCl2})$: $$ce{SO3^2- +Ba^2+ ->BaSO3 v}$$ the precipate disoolves in dilute hydrochloric acid, when sulphur dioxide evolves: $$ce{BaSO3 v +2H+ ->Ba^2+ +SO2 ^ +H2O}$$ On standing, the precipitate is slowly oxidises to the sulphate and is then …Web
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The barium sulfate precipitate is collected by filtration, dried and weighed. Since barium chloride is added in excess, and since the precipitation reaction goes to completion, we can assume that all of the sulfate is transferred from the original unknown sample to the precipitate. The mass of sulfate in the collected (ce{BaSO4}) …Web
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Answer: No, the precipitate formed is not soluble in HCl. Q6. Why does the reaction between barium chloride and sodium sulphate reach completion? Answer: The reaction between barium chloride and sodium sulphate reaches completion because it is irreversible and the white precipitate of barium sulphate is insoluble in aqueous solution. Q7.Web
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When solutions of ammonium sulfate and barium chloride are mixed, a precipitate forms. Write out the balanced molecular, total ionic, and net ionic equations for this reaction. Barium chloride reacts with sodium sulfate to precipitate barium sulfate. Balance the formula equation below and then write complete ionic and net ionic equations.Web
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Precipitation of barium sulfate has been widely studied in the past decades. Numerous theoretical and experimental research studies are reported about nucleation …Web
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The spontaneous precipitation in aqueous solutions containing relatively high barium and sulfate concentrations was investigated in the present work. In our experiments the …Web
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On adding a drop of barium chloride solution to an aqueous solution of sodium sulphite, white precipitate is obtained. ... Barium chloride on reacting with ammonium sulphate forms barium sulphate and ammonium chloride. Which of the following correctly represents the type of the reaction involved? (i) Displacement reaction ...Web
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The solution is then poured into water and then it gets a precipitate of barium sulphate. The precipitate is filtered and evaporated to get a crystalline substance, the barium sulphate or Blanc-fixe. A good cream-floated razili is about 99%. Barium sulphate with small amount of silica, iron oxide, and alumina is of white lower grades. 6.9.2 UsesWeb
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Co-precipitation of Radium with Barium and Strontium Sulfate and Its Impact on the Fate of Radium during Treatment of Produced Water from Unconventional Gas Extraction. ...Web
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Arizona State University. Barium, Ba2+ Ba 2 +. Most common oxidation state: +2. M.P. 725º. B.P. 1640º. Density 3.51 g/cm 3. Characteristics: Barium is a silvery metal. Extremely active, reacts quickly with oxygen in air, and with most non-metals.Web
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Precipitated barium sulphate is a white amorphous powder with a relative density of 4.50 (15 ℃) and a melting point of 1,580 ℃. Due to its high refractive index (1.63 to 1.65), it exhibits a ...Web
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Barium sulfate (barita) is the main commercial source of barium, although the metal will react with sulfuric acid to form the sulfate, and it can be formed from an exchange reaction (e.g., 9). The latter works because of the sulfate's low solubility in water ( K sp = 1.1 × 10 −10 ), which causes it to precipitate from solution.Web
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Abstract. Precipitation of barium sulphate in an unpremixed feed two-dimensional tubular precipitator is studied experimentally and interpreted theoretically using a closure procedure proposed previously by the authors. The closure employs the presumed beta PDF of the inert type composition variables formed with the local values of Ba and SO.Web
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The structure of the precipitate was identified by powder X-ray diffraction (PXRD), which showed that the crystals obtained using the RLFR were smaller in size than those obtained in the flask. ... The simulated volume weighted mean diameter and CSD of particles of barium sulfate were almost identical to the corresponding experimental …Web
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The K sp for strontium chromate is (3.6 times 10^{-5}) and the K sp for barium chromate is (1.2 times10^{-10}). What concentration of potassium chromate will precipitate the maximum amount of either the barium or the strontium chromate from an equimolar 0.30 M solution of barium and strontium ions without precipitating the other? …Web
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Increasing the time and decreasing the injection rate caused an increase in pressure drop and precipitation of barium sulfate salt, which was related to the …Web
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