Self-Published is not a Dirty Word

Self-Published is not a Dirty Word Self-Published is not a Dirty Word Self-Published is not a Dirty Word By Maeve Maddox In the old days, publishing companies that catered to writers who were willing to pay to have their books printed were called Vanity Presses. Family historians aside, writers who paid to publish were assumed to have failed in selling their work to a real publisher because it wasnt good enough, but they were determined to see their words in print anyway; hence the word vanity. This perception has changed along with the publishing industry. Diversity suffered when the little houses were gobbled up by the big ones. Todays conglomerates are unwilling to buy a book unless they feel it will generate a huge readership. As a result, many books that would appeal to a significant number of readers are rejected because the house doesnt think theyll appeal to a large enough audience. William P. Youngs book is a case in point. Youngs novel The Shack has been on the NY Times best seller list since June. He wrote the book as a Christmas gift for his family. They passed it around and friends urged him to publish it. One of the friends, Brad Cummings, says that Christian publishers turned it down because it was too edgy, and secular publishers turned it down because it was too Jesus-y. The book didnt fit publishers guidelines, but it has certainly hit the spot with readers. Sales of The Shack have passed the million mark and show no sign of abating. Books that sell a million copies, no matter who publishes them, are rare. According to one estimate, a major publisher considers a book a success if it sells 20,000 copies, whereas a smaller publisher might be happy with sales of 7,500 copies. Writers who make the decision to self-publish need to know what theyre getting into. Theyll have to be managers and marketers as well as writers. Theyll have to watch out for publishing scams that prey on the inexperienced. Self-publishing isnt for everyone, but it is valid way to get your book into circulation. At the least, an energetic marketer can expect to cover expenses and earn a modest profit. And theres always the possibility that the book may grab the attention of a larger public. Want to improve your English in five minutes a day? Get a subscription and start receiving our writing tips and exercises daily! Keep learning! Browse the Freelance Writing category, check our popular posts, or choose a related post below:Definitely use "the" or "a"List of 50 Great Word Games for Kids and AdultsRite, Write, Right, Wright

Calculate Solubility of AgCl From Solubility Product

Calculate Solubility of AgCl From Solubility Product This example problem demonstrates how to determine the solubility of an ionic solid in water from a substances solubility product. Problem The solubility product of silver chloride (AgCl) is 1.6 x 10-10 at 25  °C.The solubility product of barium fluoride (BaF2) is 2 x 10-6 at 25  °C. Calculate the solubility of both compounds. Solutions The key to solving solubility problems is to properly set up your dissociation reactions and define solubility. Solubility is the amount of reagent that will be consumed to saturate the solution  or reach the equilibrium of the dissociation reaction. AgCl The dissociation reaction of AgCl in water is: AgCl (s) ↔ Ag (aq) Cl- (aq) For this reaction, each mole of AgCl that dissolves produces 1 mole of both Ag and Cl-. The solubility would then equal the concentration of either the Ag or Cl ions. solubility [Ag] [Cl-] To find these concentrations, remember this formula for solubility product: Ksp [A]c[B]d So, for the reaction AB ↔ cA dB: Ksp [Ag][Cl-] Since [Ag] [Cl-]: Ksp [Ag]2 1.6 x 10-10 [Ag] (1.6 x 10-10) ½ [Ag] 1.26 x 10-5 M solubility of AgCl [Ag] solubility of AgCl 1.26 x 10-5 M BaF2 The dissociation reaction of BaF2 in water is: BaF2 (s) ↔ Ba (aq) 2 F- (aq) The solubility is equal to the concentration of the Ba ions in solution. For every mole of Ba ions formed, 2 moles of F- ions are produced, therefore: [F-] 2 [Ba] Ksp [Ba][F-]2 Ksp [Ba](2[Ba])2 Ksp 4[Ba]3 2 x 10-6 4[Ba]3 [Ba]3  ¼(2 x 10-6) [Ba]3 5 x 10-7 [Ba] (5 x 10-7)1/3 [Ba] 7.94 x 10-3 M solubility of BaF2 [Ba] solubility of BaF2 7.94 x 10-3 M Answers The solubility of silver chloride, AgCl, is 1.26 x 10-5 M at 25  °C.The solubility of barium fluoride, BaF2, is 3.14 x 10-3 M at 25  °C.