agree to the. Calculate its solubility in 0.01M NaCl aqueous solution. Click hereto get an answer to your question ️ The solubility product of AgCl in water is 1.5 × 10^-10 . x = 1.342 x 10 ^-05 moles dm^-3 = molar solubility of AgCl. community of NEET. b. A g C l is not soluble in water. Performance & security by Cloudflare, Please complete the security check to access. Calculate the solubility of AgCl in a 0.20 M AgNO3 solution. K sp = S 2. Again, these concentrations give the solubility. d. Calculate the solubility of AgCl in a 0.60 M NH 3 solution. For the precipitation of BaSO4 from the solution of BaCl2, the conc. Present in silver chloride are silver ions (A g +) and chloride ions (C l −). js.src = "//connect.facebook.net/en_US/sdk.js#xfbml=1&version=v2.10"; Calculate the solubility of AgCl (K sp = 1.8 x10-10) in pure water. Calculate the ratio of solubility of agcl in 0.1m agno3 and in pure water - 6820732 1. • Check out a … To calculate the ratio of solubility of AgCl in 0.1M AgNO^3 and in pure water what you need to put in the back of your mind is that water has a constant concentration of 1.0 x 10^-7M. Answer. Molar mass of AgCl is 143.321 g /mol. Let [Ag+] = x. … Cloudflare Ray ID: 5f8635b20c77ff38 Then [Cl-] = x, and substituting in the Ksp expression we have (x)(x) = 1.8 x 10 ^-10. The solubility product of $\ce{AgCl}$ in water is given as $1.8\cdot10^{-10}$ Determine the solubility of $\ce{AgCl}$ in pure water and in a $0.25~\mathrm{M}$ $\ce{MgSO4}$ solution. mol.wt. Want to see the step-by-step answer? Apart from being the largest NEET community, EduRev has the largest solved
The Questions and
K sp = 1.5 x 10 -10. Log in. var js, fjs = d.getElementsByTagName(s)[0]; First, write the BALANCED REACTION: Next, set up the SOLUBILITY PRODUCT EQUILIBRIUM EXPRESSION: It is given in the problem that the solubility of AgCl is 1.3 x 10-5. You may need to download version 2.0 now from the Chrome Web Store. Calculate the ratio of solubility of AgCl in .1M AgNo3 and in pure water? soon. By continuing, I agree that I am at least 13 years old and have read and
over here on EduRev! varunnair3842 varunnair3842 26.11.2018 Chemistry Secondary School Calculate the ratio of solubility of agcl in 0.1m agno3 and in pure water 2 See answers shauryakesarwani21 shauryakesarwani21 Answer: 1.34 X 10^-4. x^2 =1.8 x 10 ^-10. Does the solubility of this salt increase or decrease, compared to its solubility in pure water? Again, these concentrations give the solubility. Silver nitrate (which is soluble) has silver ion in common with silver chloride. Does the solubility of this salt increase or decrease, compared to its solubility in pure water? The solubility of insoluble substances can be decreased by the presence of a common ion. Join now. So with that information, we can say that the solubility of AgCl in 0.1M AgNO^3 is given as 0.1 M. So to determine the ratio of solubility of AgCl in 0.1M AgNO^3 and water all we need to do is; This discussion on Calculate the ratio of solubility of AgCl in .1M AgNo3 and in pure water? Ask your question. EduRev is a knowledge-sharing community that depends on everyone being able to pitch in when they know something. if (d.getElementById(id)) return; }(document, 'script', 'facebook-jssdk')); Online Chemistry tutorial that deals with Chemistry and Chemistry Concept. Join now. (function(d, s, id) { a. Calculate the solubility of AgCl in a 0.20 M AgNO3 solution. is done on EduRev Study Group by NEET Students. AgCl is 1: 1 type salt , therefore. 2) The solubility of AgCl in pure water is 1.3 x 10-5 M. Calculate the value of K sp. Solubility of AgCl will be minimum in _____. If you are on a personal connection, like at home, you can run an anti-virus scan on your device to make sure it is not infected with malware. Your IP: 37.252.96.253 1. You can study other questions, MCQs, videos and tests for NEET on EduRev and even discuss your questions like
Question bank for NEET. fjs.parentNode.insertBefore(js, fjs); L6 : Solubility in water - Sorting Materials, Science, Class 6, Solubility and Solubility product - Ionic Equilibrium, Solubility and solubility product - Ionic Equilibrium. A. Question. • If the answer is not available please wait for a while and a community member will probably answer this
Completing the CAPTCHA proves you are a human and gives you temporary access to the web property. are solved by group of students and teacher of NEET, which is also the largest student
S = √ K sp = √ 1.5x 10 -10 See Answer . Answers of Calculate the ratio of solubility of AgCl in .1M AgNo3 and in pure water? Explanation: Jamunaakailash … of [SO4—] must be greater than 1.08 x 10-8 mole/litre. js = d.createElement(s); js.id = id; To calculate the ratio of solubility of AgCl in 0.1M AgNO^3 and in pure water what you need to put in the back of your mind is that water has a constant concentration of 1.0 x 10^-7M. If you are at an office or shared network, you can ask the network administrator to run a scan across the network looking for misconfigured or infected devices. Calculate the solubility of AgCl in a 0.1 M NaCl solution. of Mg(OH)2 = 24 + (16 + 1)2 = 24 + 34 = 58, S in mole /litre = ( S in gm /litre) / mol.wt.= 9.57 x 10 -3 / 58, S is less than 0.02 , so 4S3 is neglected, S in gm / litre = 1.49 x 10 -5 x 58 = 86.42 x 10-5. because S <<< 0.1 and solubility of AgCl decreases in presence of AgNO3 due to common ion effect(common ion is Ag+).Therefore. because S <<< 0.01 and solubility of AgCl decreases in presence of NaCl due to common ion effect(common ion is Cl–).Therefore, ionic product of [Ba++] [SO4– –] > K sp of BaSO4. check_circle Expert Answer. Question 2)Solubility product of AgCl is 1.5 x 10-10 at 25 0 C . 0.01 M C a C l 2 C. Pure water. Calculate solubility of AgCl in a) pure water b) 0.1 M AgNO 3 c) 0.01 M NaCl Solution ) a) Solubility of AgCl in pure water-Solubility product ‘K sp ‘ = 1.5 x 10-10. 0.01 M N a 2 S O 4 B. The molar solubility of AgCl = [Ag+] in pure water . D. 0.001 M A g N O 3 MEDIUM. c. If 50.0 ml of 0.10M AgNO3 are added to 50.0 ml of 0.15M NaCl will a precipitate be formed? Log in. Now, let's try to do the opposite, i.e., calculate the K sp from the solubility of a salt. Another way to prevent getting this page in the future is to use Privacy Pass. Justify your answer with a calculation.