Why did the Whitechapel murders attract essays

Why did the Whitechapel murders attract essays White chapel an area between spitalfields and adlagate an area which was ignored many a time in the Victorian ages but why did it attract so much attention? Was it the intense brutality of the murders in which people felt happy and enjoyed reading about it? As jack the ripper would often use beastly methods of killing the 5 prostitutes and then take a part of their anatomy and keep it as a trophy such as in the case of Catherine Eddowes, her throat was cut and her bowels were out. her stomach was ripped up and there was a large cut from her breastbone to her stomach. Her intestines were cut out and her kidney and her womb were also cut out. There were cuts on both eyelids and the tip of her nose was cut off. This attracted so much attention because look at this the women was murdered it such a brutal way and this would have been used as an example for women to be careful and protect themselves against any strange men. This also shows that the people of Whitechapel knew what they were having to deal with. The Whitechapel murders attracted a lot of attention from the media and on two occasions letters that had been supposedly sent from the ripper were released generating more interest. Such an example was set to a Mr. Lusk and is shown below. This leeter was then later realsead to the media and in todays world prompt the question was it a hoax? Was it done to sell more newspapers? Or was it a real letter? Another point that the Whitechapel murders attracted so much attention was the whereabouts were the murders happened. The East End in 1888 was a dangerous place to be and most of the lower class lived there. There were mainly English, Poles and Jewish people living in the East End. The Jews fled from problems in Russia and had settled in the East End and were Jewish population had begun to rise slowly. Many Poles were expelled from Russia and came to live in the East End because ...

Ksp Chemistry Complete Guide to the Solubility Constant

Ksp Chemistry Complete Guide to the Solubility Constant SAT / ACT Prep Online Guides and Tips Are you learning chemistry but don’t quite understand the solubility product constant or want to learn more about it? Not sure how to calculate molar solubility from $K_s_p$? The solubility constant, or $K_s_p$, is an important part of chemistry, particularly when you’re working with solubility equations or analyzing the solubility of different solutes. When you have a solid grasp of $K_s_p$, those questions become much easier to answer! In this $K_s_p$ chemistry guide, we’ll explain the $K_s_p$ chemistry definition, how to solve for it (with examples), which factors affect it, and why it’s important. At the bottom of this guide, we also have a table with the $K_s_p$ values for a long list of substances to make it easy for you to find solubility constant values. What Is $K_s_p$? $K_s_p$ is known as the solubility constant or solubility product. It’s the equilibrium constant used for equations when a solid substance is dissolving in a liquid/aqueous solution. As a reminder, a solute (what is being dissolved) is considered soluble if more than 1 gram of it can be completely dissolved in 100 ml of water. $K_s_p$ is used for solutes that are only slightly soluble and don’t completely dissolve in solution. (A solute is insoluble if nothing or nearly nothing of it dissolves in solution.) $K_s_p$ represents how much of the solute will dissolve in solution. The value of $K_s_p$ varies depending on the solute. The more soluble a substance is, the higher its $K_s_p$ chemistry value. And what are the $K_s_p$ units? Actually, it doesn’t have a unit! The $K_s_p$ value does not have any units because the molar concentrations of the reactants and products are different for each equation. This would mean the $K_s_p$ unit would be different for every problem and would be difficult to solve, so in order to make it simpler, chemists generally drop $K_s_p$ units altogether. How nice of them! How Do You Calculate $K_s_p$? In this section, we explain how to write out $K_s_p$ chemistry expressions and how to solve for the value of $K_s_p$. For most chemistry classes, you’ll rarely need to solve for the value of $K_s_p$; most of the time you’ll be writing out the expressions or using $K_s_p$ values to solve for solubility (which we explain how to do in the â€Å"Why Is $K_s_p$ Important† section). Writing $K_s_p$ Expressions Below is the solubility product equation which is followed by four $K_s_p$ chemistry problems so you can see how to write out $K_s_p$ expressions. For the reaction $A_aB_b$(s) â‡Å' $aA^b^{+}$(aq) + $bB^a^{-}$ (aq) The solubility expression is $K_s_p$= $[A^b^{+}]^a$ $[B^a^{-}]^b$ The first equation is known as a dissociation equation, and the second is the balanced $K_s_p$ expression. For these equations: A and B represent different ions and solids. In these equations, they are also referred to as "products". a and b represent coefficients used to balance the equation (aq) and (s) indicate which state the product is in (aqueous or solid, respectively) Brackets stand for molar concentration. So [AgCl] represents the molar concentration of AgCl. In order to write $K_s_p$ expressions correctly, you need to have a good knowledge of chemical names, polyatomic ions, and the charges associated with each ion. Also, the key thing to be aware of with these equations is that each concentration (represented by square brackets) is raised to the power of its coefficient in the balanced $K_s_p$ expression. Let’s look at a few examples. Example 1 $PbBr_2$(s) â‡Å' $Pb^2^{+}$ (aq) + $2Br^{ ¯}$ (aq) $K_s_p$= $[Pb^2^{+}]$ $[Br ¯]^2$ In this problem, don’t forget to square the Br in the $K_s_p$ equation. You do this because of the coefficient â€Å"2† in the dissociation equation. Example 2 CuS(s) â‡Å' $Cu^{+}$ (aq) + S ¯(aq) $K_s_p$= [$Cu^{+}$] [S ¯] Example 3 $Ag_2CrO_4$ (s) â‡Å' 2$Ag^{+}$ (aq) + $CrO_4^2^{-}$ (aq) $K_s_p$= $[Ag^{+}]^2$ [$CrO_4^2$] Example 4 $Cu_3$ $(PO_4)^2$ (s) â‡Å' $3Cu^2^{+}$ (aq) + $2PO_4^3^{ ¯}$ (aq) $K_s_p$ = $[Cu^2^{+}]^3$ [$PO_4^3^ ¯$]$^2$ Solving for $K_s_p$ With Solubility In order to calculate a value for $K_s_p$, you need to have molar solubility values or be able to find them. Question: Determine the $K_s_p$ of AgBr (silver bromide), given that its molar solubility is 5.71 x $10^{ ¯}^7$ moles per liter. First, we need to write out the two equations. AgBr(s) â‡Å' $Ag^{+}$ (aq) + $Br^{ ¯}$ (aq) $K_s_p$ = [$Ag^{+}$] [$Br^{ ¯}$] Now, since in this problem we're solving for an actual value of $K_s_p$, we plug in the solubility values we were given: $K_s_p$ = (5.71 x $10^{ ¯}^7$) (5.71 x $10^{ ¯}^7$) = 3.26 x $10^{ ¯}^13$ The value of $K_s_p$ is 3.26 x $10^{ ¯}^13$ What Factors Affect $K_s_p$? In this section, we discuss the main factors that affect the value of the solubility constant. Temperature Most solutes become more soluble in a liquid as the temperature is increased. If you’d like proof, see how well instant coffee mixes in a cup of cold water compared to a cup of hot water. Temperature affects the solubility of both solids and gases but hasn’t been found to have a defined impact on the solubility of liquids. Pressure Pressure can also affect solubility, but only for gases that are in liquids. Henry's law states that the solubility of a gas is directly proportional to the partial pressure of the gas. Henry’s law is written as p=kc, where p is the partial pressure of the gas above the liquid k is Henry’s law constant c is the concentration of gas in the liquid Henry’s law shows that, as partial pressure decreases, the concentration of gas in the liquid also decreases, which in turn decreases solubility. So less pressure results in less solubility, and more pressure results in more solubility. You can see Henry’s law in action if you open up a can of soda. When the can is closed, the gas is under more pressure, and there are lots of bubbles because a lot of the gas is dissolved. When you open the can, the pressure decreases, and, if you leave the soda sitting out long enough, the bubbles will eventually disappear because solubility has decreased and they are no longer dissolved in the liquid (they’ve bubbled out of the drink). Molecular Size Generally, solutes with smaller molecules are more soluble than ones with molecules particles. It’s easier for the solvent to surround smaller molecules, so those molecules can be dissolved faster than larger molecules. Why Is $K_s_p$ Important? Why does the solubility constant matter? Below are three key times you’ll need to use $K_s_p$ chemistry. To Find the Solubility of Solutes Wondering how to calculate molar solubility from $K_s_p$? Knowing the value of $K_s_p$ allows you to find the solubility of different solutes. Here’s an example: The $K_s_p$ value of $Ag_2SO_4$ ,silver sulfate, is 1.4Ãâ€"$10^{–}^5$. Determine the molar solubility. First, we need to write out the dissociation equation: $K_s_p$=$ [Ag^{+}]^2$ $[SO_4^2]$ Next, we plug in the $K_s_p$ value to create an algebraic expression. 1.4Ãâ€"$10^{–}^5$= $(2x)^2$ $(x)$ 1.4Ãâ€"$10^{–}^5$= $4x^3$ $x$=[$SO_4^2$]=1.5x$10^{-}^2$ M $2x$= [$Ag^{+}$]=3.0x$10^{-}^2$ M To Predict If a Precipitate Will Form in Reactions When we know the $K_s_p$ value of a solute, we can figure out if a precipitate will occur if a solution of its ions is mixed. Below are the two rules that determine the formation of a precipitate. Ionic product $K_s_p$ then precipitation will occur Ionic product $K_s_p$ then precipitation will not occur To Understand the Common Ion Effect $K_s_p$ also is an important part of the common ion effect. The common ion effect states that when two solutions that share a common ion are mixed, the solute with the smaller $K_s_p$ value will precipitate first. For example, say BiOCl and CuCl are added to a solution. Both contain $Cl^{-}$ ions. BiOCl’s $K_s_p$ value is 1.8Ãâ€"$10^{–}^31$ and CuCl’s $K_s_p$ value is 1.2Ãâ€"$10^{–}^6$. BiOCl has the smaller $K_s_p$ value, so it will precipitate before CuCl. Solubility Product Constant Table Below is a chart showing the $K_s_p$ values for many common substances. The $K_s_p$ values are for when the substances are around 25 degrees Celsius, which is standard. Because the $K_s_p$ values are so small, there may be minor differences in their values depending on which source you use. The data in this chart comes from the University of Rhode Island’s Department of Chemistry. Substance Formula $K_s_p$ Value Aluminum hydroxide $Al(OH)_3$ 1.3Ãâ€"$10^{–}^33$ Aluminum phosphate $AlPO_4$ 6.3Ãâ€"$10^{–}^19$ Barium carbonate $BaCO_3$ 5.1Ãâ€"$10^{–}^9$ Barium chromate $BaCrO_4$ 1.2Ãâ€"$10^{–}^10$ Barium fluoride $BaF_2$ 1.0Ãâ€"$10^{–}^6$ Barium hydroxide $Ba(OH)_2$ 5Ãâ€"$10^{–}^3$ Barium sulfate $BaSO_4$ 1.1Ãâ€"$10^{–}^10$ Barium sulfite $BaSO_3$ 8Ãâ€"$10^{–}^7$ Barium thiosulfate $BaS_2O_3$ 1.6Ãâ€"$10^{–}^6$ Bismuthyl chloride $BiOCl$ 1.8Ãâ€"$10^{–}^31$ Bismuthyl hydroxide $BiOOH$ 4Ãâ€"$10^{–}^10$ Cadmium carbonate $CdCO_3$ 5.2Ãâ€"$10^{–}^12$ Cadmium hydroxide $Cd(OH)_2$ 2.5Ãâ€"$10^{–}^14$ Cadmium oxalate $CdC_2O_4$ 1.5Ãâ€"$10^{–}^8$ Cadmium sulfide $CdS$ 8Ãâ€"$10^{–}^28$ Calcium carbonate $CaCO_3$ 2.8Ãâ€"$10^{–}^9$ Calcium chromate $CaCrO_4$ 7.1Ãâ€"$10^{–}^4$ Calcium fluoride $CaF_2$ 5.3Ãâ€"$10^{–}^9$ Calcium hydrogen phosphate $CaHPO_4$ 1Ãâ€"$10^{–}^7$ Calcium hydroxide $Ca(OH)_2$ 5.5Ãâ€"$10^{–}^6$ Calcium oxalate $CaC_2O_4$ 2.7Ãâ€"$10^{–}^9$ Calcium phosphate $Ca_3(PO_4)_2$ 2.0Ãâ€"$10^{–}^29$ Calcium sulfate $CaSO_4$ 9.1Ãâ€"$10^{–}^6$ Calcium sulfite $CaSO_3$ 6.8Ãâ€"$10^{–}^8$ Chromium (II) hydroxide $Cr(OH)_2$ 2Ãâ€"$10^{–}^16$ Chromium (III) hydroxide $Cr(OH)_3$ 6.3Ãâ€"$10^{–}^31$ Cobalt (II) carbonate $CoCO_3$ 1.4Ãâ€"$10^{–}^13$ Cobalt (II) hydroxide $Co(OH)_2$ 1.6Ãâ€"$10^{–}^15$ Cobalt (III) hydroxide $Co(OH)_3$ 1.6Ãâ€"$10^{–}^44$ Cobalt (II) sulfide $CoS$ 4Ãâ€"$10^{–}^21$ Copper (I) chloride $CuCl$ 1.2Ãâ€"$10^{–}^6$ Copper (I) cyanide $CuCN$ 3.2Ãâ€"$10^{–}^20$ Copper (I) iodide $CuI$ 1.1Ãâ€"$10^{–}^12$ Copper (II) arsenate $Cu_3(AsO_4)_2$ 7.6Ãâ€"$10^{–}^36$ Copper (II) carbonate $CuCO_3$ 1.4Ãâ€"$10^{–}^10$ Copper (II) chromate $CuCrO_4$ 3.6Ãâ€"$10^{–}^6$ Copper (II) ferrocyanide $Cu[Fe(CN)_6]$ 1.3Ãâ€"$10^{–}^16$ Copper (II) hydroxide $Cu(OH)_2$ 2.2Ãâ€"$10^{–}^20$ Copper (II) sulfide $CuS$ 6Ãâ€"$10^{–}^37$ Iron (II) carbonate $FeCO_3$ 3.2Ãâ€"$10^{–}^11$ Iron (II) hydroxide $Fe(OH)_2$ 8.0$10^{–}^16$ Iron (II) sulfide $FeS$ 6Ãâ€"$10^{–}^19$ Iron (III) arsenate $FeAsO_4$ 5.7Ãâ€"$10^{–}^21$ Iron (III) ferrocyanide $Fe_4[Fe(CN)_6]_3$ 3.3Ãâ€"$10^{–}^41$ Iron (III) hydroxide $Fe(OH)_3$ 4Ãâ€"$10^{–}^38$ Iron (III) phosphate $FePO_4$ 1.3Ãâ€"$10^{–}^22$ Lead (II) arsenate $Pb_3(AsO_4)_2$ 4Ãâ€"$10^{–}^6$ Lead (II) azide $Pb(N_3)_2$ 2.5Ãâ€"$10^{–}^9$ Lead (II) bromide $PbBr_2$ 4.0Ãâ€"$10^{–}^5$ Lead (II) carbonate $PbCO_3$ 7.4Ãâ€"$10^{–}^14$ Lead (II) chloride $PbCl_2$ 1.6Ãâ€"$10^{–}^5$ Lead (II) chromate $PbCrO_4$ 2.8Ãâ€"$10^{–}^13$ Lead (II) fluoride $PbF_2$ 2.7Ãâ€"$10^{–}^8$ Lead (II) hydroxide $Pb(OH)_2$ 1.2Ãâ€"$10^{–}^15$ Lead (II) iodide $PbI_2$ 7.1Ãâ€"$10^{–}^9$ Lead (II) sulfate $PbSO_4$ 1.6Ãâ€"$10^{–}^8$ Lead (II) sulfide $PbS$ 3Ãâ€"$10^{–}^28$ Lithium carbonate $Li_2CO_3$ 2.5Ãâ€"$10^{–}^2$ Lithium fluoride $LiF$ 3.8Ãâ€"$10^{–}^3$ Lithium phosphate $Li_3PO_4$ 3.2Ãâ€"$10^{–}^9$ Magnesium ammonium phosphate $MgNH_4PO_4$ 2.5Ãâ€"$10^{–}^13$ Magnesium arsenate $Mg_3(AsO_4)_2$ 2Ãâ€"$10^{–}^20$ Magnesium carbonate $MgCO_3$ 3.5Ãâ€"$10^{–}^8$ Magnesium fluoride $MgF_2$ 3.7Ãâ€"$10^{–}^8$ Magnesium hydroxide $Mg(OH)_2$ 1.8Ãâ€"$10^{–}^11$ Magnesium oxalate $MgC_2O_4$ 8.5Ãâ€"$10^{–}^5$ Magnesium phosphate $Mg_3(PO_4)_2$ 1Ãâ€"$10^{–}^25$ Manganese (II) carbonate $MnCO_3$ 1.8Ãâ€"$10^{–}^11$ Manganese (II) hydroxide $Mn(OH)_2$ 1.9Ãâ€"$10^{–}^13$ Manganese (II) sulfide $MnS$ 3Ãâ€"$10^{–}^14$ Mercury (I) bromide $Hg_2Br_2$ 5.6Ãâ€"$10^{–}^23$ Mercury (I) chloride $Hg_2Cl_2$ 1.3Ãâ€"$10^{–}^18$ Mercury (I) iodide $Hg_2I_2$ 4.5Ãâ€"$10^{–}^29$ Mercury (II) sulfide $HgS$ 2Ãâ€"$10^{–}^53$ Nickel (II) carbonate $NiCO_3$ 6.6Ãâ€"$10^{–}^9$ Nickel (II) hydroxide $Ni(OH)_2$ 2.0Ãâ€"$10^{–}^15$ Nickel (II) sulfide $NiS$ 3Ãâ€"$10^{–}^19$ Scandium fluoride $ScF_3$ 4.2Ãâ€"$10^{–}^18$ Scandium hydroxide $Sc(OH)_3$ 8.0Ãâ€"$10^{–}^31$ Silver acetate $Ag_2CH_3O_2$ 2.0Ãâ€"$10^{–}^3$ Silver arsenate $Ag_3AsO_4$ 1.0Ãâ€"$10^{–}^22$ Silver azide $AgN_3$ 2.8Ãâ€"$10^{–}^9$ Silver bromide $AgBr$ 5.0Ãâ€"$10^{–}^13$ Silver chloride $AgCl$ 1.8Ãâ€"$10^{–}^10$ Silver chromate $Ag_2CrO_4$ 1.1Ãâ€"$10^{–}^12$ Silver cyanide $AgCN$ 1.2Ãâ€"$10^{–}^16$ Silver iodate $AgIO_3$ 3.0Ãâ€"$10^{–}^8$ Silver iodide $AgI$ 8.5Ãâ€"$10^{–}^17$ Silver nitrite $AgNO_2$ 6.0Ãâ€"$10^{–}^4$ Silver sulfate $Ag_2SO_4$ 1.4Ãâ€"$10^{–}^5$ Silver sulfide $Ag_2S$ 6Ãâ€"$10^{–}^51$ Silver sulfite $Ag_2SO_3$ 1.5Ãâ€"$10^{–}^14$ Silver thiocyanate $AgSCN$ 1.0Ãâ€"$10^{–}^12$ Strontium carbonate $SrCO_3$ 1.1Ãâ€"$10^{–}^10$ Strontium chromate $SrCrO_4$ 2.2Ãâ€"$10^{–}^5$ Strontium fluoride $SrF_2$ 2.5Ãâ€"$10^{–}^9$ Strontium sulfate $SrSO_4$ 3.2Ãâ€"$10^{–}^7$ Thallium (I) bromide $TlBr$ 3.4Ãâ€"$10^{–}^6$ Thallium (I) chloride $TlCl$ 1.7Ãâ€"$10^{–}^4$ Thallium (I) iodide $TlI$ 6.5Ãâ€"$10^{–}^8$ Thallium (III) hydroxide $Tl(OH)_3$ 6.3Ãâ€"$10^{–}^46$ Tin (II) hydroxide $Sn(OH)_2$ 1.4Ãâ€"$10^{–}^28$ Tin (II) sulfide $SnS$ 1Ãâ€"$10^{–}^26$ Zinc carbonate $ZnCO_3$ 1.4Ãâ€"$10^{–}^11$ Zinc hydroxide $Zn(OH)_2$ 1.2Ãâ€"$10^{–}^17$ Zinc oxalate $ZnC_2O_4$ 2.7Ãâ€"$10^{–}^8$ Zinc phosphate $Zn_3(PO_4)_2$ 9.0Ãâ€"$10^{–}^33$ Zinc sulfide $ZnS$ 2Ãâ€"$10^{–}^25$ Conclusion: $K_s_p$ Chemistry Guide What is $K_s_p$ in chemistry? The solubility product constant, or $K_s_p$, is an important aspect of chemistry when studying solubility of different solutes. $K_s_p$ represents how much of the solute will dissolve in solution, and the more soluble a substance is, the higher the chemistry $K_s_p$ value. To calculate the solubility product constant, you’ll first need to write out the dissociation equation and balanced $K_s_p$ expression, then plug in the molar concentrations, if you’re given them. The solubility constant can be affected by temperature, pressure, and molecular size, and it’s important for determining solubility, predicting if a precipitate will form, and understand the common ion effect.