Which of the following is the correct solubility product constant for the reaction shown below? NEET 2018: The solubility of BaSO4 in water is 2.42 × 10-3 gL-1 at 298 K. The value of its solubility product (Ksp) will be (Given molar mass of B 1.08 x 10-14 mol 2 L-2 Equilibrium. Following solutions were prepared by mixing different volumes of $\ce{NaOH}$ and $\ce{HCl}$ of different concentrations: On which of the following properties does the coagulating power of an ion depend ? What is the solubility of BaSO4 in water, in moles per litre? A solution has a [Ca2+] of 0.00350 M. What concentration of hydroxide is needed before precipitation begins? Considering Ellingham diagram, which of the following metals can be used to reduce alumina ? Organic Chemistry – Some Basic Principles and Techniques, General Principles and Processes of Isolation of Elements, Classification of Elements and Periodicity in Properties, The solubility of BaSO4 in water is 2.42 × 10-3 gL-1 at 298 K. The value of its solubility product (Ksp) will be (Given molar mass of BaSO4 = 233 g mol-1). This relationship also facilitates finding the $$K_{sq}$$ of a slightly soluble solute from its solubility. What is the Ksp for the following reaction, if the concentration of Ba2+ was measured to be 0.0075 M and F− was measured to be 0.015 M? A solution has [Zn2+] of 8.9 × 10-4 M and 0.100 M NH3. Ksp of PbCl2 = 1.17 × 10-5. Kf of Ag(S2O3)23−. The reaction : $\ce{N2O4 <=> 2NO2}$, An aqueous solution contains $0.10 \, M \, H_2S$ and $0.20 \, M \, HCl$ . What equation best represents the behavior of BaSO4 in water? Ksp of Ca(OH)2 = 4.68 × 10-6. What equation best represents the behavior of PbSO4 in water? What is the concentration of Zn2+ after the solution reaches equilibrium? What is the molar solubility of Ca(OH)2 if the Ksp is 6.5 × 10-6? 5.5 × 10–11 mol… Ksp of Ag2CrO4 = 1.12 × 10-12. What concentration of Cu2+ is needed to have a concentration of Cu(CN)42- equal to 2.0 × 10-5 M in a solution with [CN−] is 9.3 × 10-4 M? The solubility product (Ksp) of BaSO4 is 1.1x10^-10 at 25*C. What is the solubility of BaSO4? What is the Ksp for the following reaction if the concentration of Pb2+ was measured to be 0.0043 M and F− was measured to be 0.0029 M. If the equilibrium constants for the formation of $HS^-$ from $H_2S$ is $1.0 \times 10^{-7}$ and that of $S^{2- }$ from $HS^-$ ions is $1.2 \times 10^{-13}$ then the concentration of $S^{2-}$ ions in aqueous solution is -, At 320 K, a gas A2 is 20% dissociated to A(g). Which of the following statements is not true for halogens? (R = alkyl), The solubility of $\ce{BaSO_4}$ in water is $2.42 \times 10^{-3} \, gL^{-1}$ at 298 K. The value of its solubility product $(K_{sp})$ will be. b. I am going to assume that you are given the solubility of an ionic compound in mol dm-3. We decide to reduce the solubility of BaSO4 in water by adding in sodium sulafate. Given van der Waals' constant for $\ce{NH_3 , H_2 , O_2}$ and $\ce{CO_2}$ are respectively 4.17, 0.244, 1.36 and 3.59, which one of the following gases is most easily liquefied ? 1.08 x 10-12 mol 2 L-2. Chapter 17 practice test. The solubility of BaSO4 in water is 2.42 x 10-3 g L-1 at 298 K. The value of its solubility product (Ksp) will be (Given molar mass of BaSO4 = 233 g mol-1) (a) 1.08 x 10-10 mol2 L-2. A solution has [Ag+] of 2.9 × 10-4 M and 0.225 M of (S2O3)2−. Identify compound X in the following sequence of reactions: Identify a molecule which does not exist. Solution for The solubility product, Ksp, for BaSO4 is 1.1 × 10–10. Which of the following set of molecules will have zero dipole moment ? Click hereto get an answer to your question ️ If the solubility product of BaSO4 is 1.5 × 10^-10 in water. We decide to reduce the solubility of BaSO4 in water by adding in sodium sulafate. (b) 1.08 x 10-12 mol2 L-2. On electrolysis of dil.sulphuric acid using Platinum (Pt) electrode, the product obtained at anode will be: An element has a body centered cubic (bcc) structure with a cell edge of 288 pm. The solubility of barium sulphate at 298 K is 1.05 x 10-5 mol dm-3. A) What Would Be The Solubility Be In (1) H20 Alone (ii) A 0.003 Mol Dm Solution Of BaCl2 (iii) A 0.006 Mol Dm Solution Of Na2SO4 ? What equation best represents the behavior of solid Mg(OH)2 when added to water? Which of the following carbocations is expected to be most stable ? 69 terms. Which of the following is the correct solubility product constant for the reaction shown below? What is the molar solubility of AgCl if the Ksp is 1.8 × 10-10? Kf of Pb(OH)2 = 8.0 × 1013. The decomposition of $\ce{N2O4}$, in equilibrium mixture of $\ce{NO2(g)}$ and $\ce{N2O4(g)}$, can be increased by : In Wolff‐Kishner reduction, the carbonyl group of aldehydes and ketones is converted into. Select one: a. Of BaSO4 In Water Is 1.3x10-10 At 25°C. Which equation best represents the formation of AlF63-? What is the concentration of Ag+ after the solution reaches equilibrium? If it was in g dm-3, or any other concentration units, you would first have to convert it into mol dm-3. A solution has a [Pb2+] of 0.00105 M. What concentration of chloride is needed before precipitation begins? Which of the following is correct with respect to $- I$ effect of the substituents ? Given that the ionic product of $Ni(OH)_2$ is $2 \times 10^{-15}$. The gas phase reaction $\ce{2NO2(g) -> N2O4(g)}$ is an exothermic reaction. 1.08 x 10-8 mol 2 L-2. What will be the solubility of BaSO4 in a 0.010 M solution of NaSO4? Ksp = 1.1 10-10. Ksp of FeS = 3.72 × 10-10, A solution has [Ag+] of 3.2 × 10-3 M and 0.125 M NH3. Solubility product / Constant concentration of Barium Ions in the solutions = 1.08*10^-10 / 0.001 = 1.08*10^-10/10^-3 = 1.08*10^-7 molar. When the solution becomes saturated with ions, that is, unable to hold any more, the excess solid settles to the bottom of the container and an equilibrium is established between the undissolved solid and the dissolved ions. Chemistry. The solubility product of B... chemistry. What will be the equilibrium constant of the given reaction carried out in a $5 \,L$ vessel and having equilibrium amounts of $A_2$ and $A$ as $0.5$ mole and $2 \times 10^{-6}$ mole respectively ? asked Dec 20, 2018 in Equilibrium by monuk (68.0k points) recategorized Feb 11 by subrita. Its solubility, in moles per litre, is. Get more help from Chegg . = 2.9 × 1013. A sample of $HI_{(g)}$ is placed in a flask at a pressure of $0.2$ atm. The solubility product (K sp) of BaSO 4 is 1.5 X 10-9.Calculate the solubility of barium sulphate in pure water and in 0.1 M BaCl 2. Kf of Ag(NH3)2+ = 1.7 × 107. 92 terms. b. It is clear that if the concentration of Sulphate ions is any higher than this Val then, the ionic product of barium sulphate in the solution (viz. What equation best represents the behavior of BaSO4 in water? (a) $CO_2(g)$ is used as refrigerant for ice-cream and frozen food. The solubility product of BaSO4 is 1.5 × 10^-9 at 18^oC . What is the molar solubility of NiS if the Ksp is 3.0 × 10-20? The solubility of BaSO 4 in water is 2.42 × 10 –3 gL –1 at 298 K. The value of its solubility product (K sp) will be (Given the molar mass of BaSO 4 = 233 g mol –1) 1.08 x 10-10 mol 2 L-2. What will be the solubility of BaSO4 in a 0.010 M solution of NaSO4? The atomic radiusis: Find out the solubility of $Ni(OH)_2$ in 0.1 M NaOH. Select one: a. Solubility Equilibria. Reaction between acetone and methyl magnesium chloride followed by hydrolysis will give : Identify the correct statements from the following: B) Would Precipitation Of BaSO4 Occur If 25cm Of 0.001 Mol Dm BaCl2 Were Mixed With 75cm Of 0.002 Mol Dm Na2SO4 ? The solubility product, Ksp, for BaSO4 is 1.1 * 10-10. Solubility product constants ($$K_{sq}$$) are given to those solutes, and these constants can be used to find the molar solubility of the compounds that make the solute. Calculating solubilities from solubility products. What will be the expression of $K_p$ for the given reaction if the total pressure inside the vessel is $P$ and degree of dissociation of the reactant is $a$ ? Calculating solubility products from solubilities. Solution Show Solution (i) Let the solubility of BaSO 4 in pure water be x mol/L What is the Ksp for the following reaction, if the concentration of Fe2+ was measured to be 5.8 x 10-6 M and OH− was measured to be 1.16 x 10-5 M? Which of the following is the correct solubility product constant for the following reaction? Introduction. What is the molar solubility of Cr(OH)3 if the Ksp is 1.6 × 10-30? The standard free energy change at 320 K and 1 atm in J mol$^{-1}$ is approximately : (R=8.314 JK$^{-1}$ mol$^{-1}$; ln 2=0.693; ln 3=1.098). a. A solution has a [Ag+] of 0.00175 M. What concentration of chromate is needed before precipitation begins?