Thermochemistry Heat of precipitation - precipitate is unsoluble salt - precipitate must be prepared through double bond decomposition or precipitation method Do you still remember what is meant by double bond decomposition? [please refer to salts notes] General equation double bond decomposition/precipitation; Ionic equation for precipitation reaction. Salt Solubility in water Li+‚ Na+‚ K+‚ NH4+ All salt dissolve in water Nitrate‚ NO3- All nitrate salt
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fertilizer 15 Calcium oxide CaO Used to make plaster 16 Carbon dioxide CO2 Dry ice 17 Chromium oxide Cr2O3 Green pigment in paints 18 Copper sulfate CuSO4 Plant root killer 19 Iron(III) chloride FeCl3 Etching solution 20 Magnesium carbonate MgCO3 Athlete’s chalk 21 Mg(OH)2 Milk of Magnesia 22 Dinitrogen oxide Gas in whipped cream cans 23 Potassium nitrate KNO3 Saltpeter 24 Potassium permanganate KMnO4 Used in water softeners B. Follow-Up Questions: Part I 1. How are isotopes of an element different
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http://foricseandbeyond.blogspot.in/ DE’S FOUNDATION BISTUPUR‚ JSR ACTION OF HEAT ON CHEMICAL COMPOUNDS “Analytical chemistry -I” http://foricseandbeyond.blogspot.in/ metal oxide “Oxides of metals are generally stable to heat and they are considered to be most stable form of compound found in nature.” Oxides of potassium‚sodium‚calcium‚magnesium‚ aluminum ‚ zinc‚iron‚lead and copper are stable to heat uO C PbO Zn O http://foricseandbeyond.blogspot.in/ MERCURIC OXIDE
Free Oxide Oxygen Nitrogen
of the following combinations of solutions yields a precipitate? A. B. C. D. E. KNO3(aq) and CaCl2(aq) AgNO3(aq) and NH4Br(aq) Mg(NO3)2(aq) and Li2SO4(aq) More than one of these combinations yields a precipitate. None of these combinations yields a precipitate. 7. (0.5 marks) Is the reaction below a precipitation‚ an acid-base or an oxidation-reduction reaction? Assume the reaction occurs in aqueous solution. CuSO4 + Zn → Cu + ZnSO4 A. B. C. a precipitation reaction an acid-base reaction an oxidation-reduction
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CHM130 Lab 5 The Atomic Mass of Beanium Name: Paige Miller A. Data Table: Insert your Data Table here with your sample calculations. You must show at least one sample calculation per procedure step. (16 points) Part I Data Table Sample Mass (mg) Number/Qty Average Mass (mg) Relative Abundance Relative Weight (mg) Kidneybeanium 1660.00 mg 3 553.33 mg 0.2143 118.58 mg Pintobeanium 2830.00 mg 6 471.67 mg 0.4286 202.16 mg Blackeyedpeaium 1110.00 mg 5 222.00 mg
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Ammonium sulphate (NH4)2SO4. FW = 132.14‚ Eq. = 66g/l. 250ml 0.05M = 1.325g = 0.1N | Adipic acid HO2C(CH2)4CO2H‚ FW = 146.4‚ Eq. = 73.03g/l 250ml 0.05M = 1.83g = 0.1N | Barium hydroxide Ba(OH)2.8H2O‚ FW = 315.48‚ Eq. = 157.5g/l 250ml 0.05M = 3.94g = 0.1N | Benzoic acid C6H5COOH‚ FW = 122.12‚ Eq. = 61g/l 250ml 0.05M = 1.52g = 0.1N | Calcium carbonate CaCO3‚ FW = 100.00‚ Eq. = 50g/l 250ml 0.05M = 1.25g = 0.1N | Furroic acid FW = 112.08‚ Eq. = 112g/l 250ml 0.1M = 2.8g = 0.1N |
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Abstract In this experiment‚ you will study the effect of changing temperature on the amount of solutet will dissolve in a given amount of water. In this experiment‚ you will completely dissolve different quantities of potassium nitrate‚ KNO3‚ in the same volume of water at a high temperature. As each solution cools‚ you will monitor temperature using a computer-interfaced Temperature Probe and observe the precise instant that solid crystals start to form. At this moment‚ the solution is
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K3Fe(CN)6(aq) ↔ KFe(III)Fe(II)(CN)6(s) + 2K+(aq) To determine the presence of Fe3+‚ 0.10 M of KSCN was used. The product was a blood red solution. The reaction’s balanced equation is: Fe(NO3)2 (aq) + 2 KSCN (aq) Fe(SCN)2 (aq) + 2 KNO3 (aq) It has a net ionic equation of: Fe3+(aq) + SCN-(aq) → FeSCN2+(aq) 1.00 M HCl‚ meanwhile‚ was used to determine the presence of Ag+ in the resulting supernate. This resulted to formation of white
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temperature rises‚ the solubility of KNO3 also rises 4. Temperature C | Your data KNO3 in grams per 100 ml of H2O | CCZ data KNO3 in grams per 100ml of H2O | 35 C | 49 | 49 | 35 C | 49 | 49 | 70 C | 135 | 180 | 5. Data pointGrams of KNO3 in grams per 100ml of H2O at C | Your data saturated‚ unsaturated or supersaturated | CCZ data saturated‚ unsaturated or supersaturated | 75g of KNO3/100g H2O at 40 C | Saturated | Not saturated | 60g of KNO3 /100g H2O at 50 C | Not saturated
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that decreasing the temperature of the system will increase the solubility of gases. In this experiment‚ the effect of temperature on the solubility of potassium nitrate‚ KNO3‚ in the universal solvent‚ water‚ will be analyzed. Purpose: To determine the effect of temperature on the solubility of potassium nitrate‚ KNO3‚ in water. General Safety: * Goggles * Use test tube holders when removing test tubes from hot water bath * Use gloves to remove hot water bath from hot plate
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