NaHCO3‚ Na3PO4 and CH3COOH. In order of increasing pH: Here are my predictions: ACIDS - H2SO4 – - HCL – - H2SO3 – Weak Acid; - CH3COOH – Weak Acid; - NH4Cl – Weak Acid; - HCN- Weak Acid; NEUTRAL - KNO3 – This is neutral BASES - NaCH3COO – This is a weak base; - NaHCO3 –Weak Base; - NaCN – Weak Base; - NH3 – Weak Base; - Na3PO4 - Weak
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Chemistry 200 Exam 1 Review Problems 1. Calculate the number of atoms in 10.0 grams of Fe. 2. Give the mass number‚ #protons‚ #neutrons and #electrons for the isotope strontium-88. 3. Calculate the number of moles of carbon in 50.0 g of benzene C6H6 4. A substance is found to be 38.7 % C‚ 9.7 % H and 51.6 % O by mass. Its molar mass is 62.1 g/mole. What is its molecular formula? 5. Name the following: a) Ca(OH)2 b) KCN c) HClO4(aq) d) FeSO4 e) Na2O f) SF6 g)
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Lab Report 1 Introduction: Proper chemical formulas entitle many challenges such as the Law of Multiple proportions that states that there may be more than one plausible mole ratio for the elements in that compound. However if we determine the mass of each element in the compound we will be able to get the true chemical formula. In this experiment‚ we used the law of definite proportions to find the chemical formula for a hydrated compound containing copper‚ chlorine‚ and water molecules
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Unit 2 Online Simulation-II (50 points) VLab: Precipitation Reactions: Data & Observations Navigate to: http://www.sascurriculumpathways.com/portal/#/search?searchString=&searchSubject=3&searchCategory=20 Enter the following username: job5circle (No password required) Enter 867 GO There are thirty-five combinations of aqueous solutions for you to investigate. (Note Table 1 on the Data Sheet.) Some of these combinations will produce precipitates; others will not. Step-by-step
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electrons in the samples and observe the color of the flame. The flame emits a color because each element has an exactly defined emission spectrum‚ which one can use to identify them. For example‚ NaCl was highlighter yellow‚ Sr(NO3)2 was sun orange‚ CuCl2 was turquoise‚ LiCl was neon red‚ KCl was solar flare yellow‚ and BaCl2 was Voldemort green. Introduction- In Bohr’s model of the atom‚ electrons travel around the nucleus in an orbit. The concentric circles in his model represent the energy levels
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CHEMICAL REACTION (SYNTHESIS REACTION‚ DECOMPOSITION AND SINGLE REAPLACEMENT REACTION) Purpose : 1. To identify the chemical changes 2. To observe the effect of temperature of a chemical reaction. Theoritical basic : A chemical reaction is a process that leads to the transformation of one set of chemical substances to another. Classically‚ chemical reactions encompass changes that strictly involve the motion of electrons in the forming and breaking of chemical bonds between
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Experiments #7A & 7B 7A. Electrochemical Cells 7B. Formation of a Complex Ion Chem 102 Section 3095 Grace H. Kim Dec. 15‚ 2011 Abstract Two experiments were conducted to figure out the value of the formation constant of tetraamminecopper(II)‚ Kf‚ with different methods and which experimental method produces more accurate result. One was electrochemistry using a Daniel cell and the other one was spectrometry by estimating concentration of complex solution using a calibration
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Purpose/Objective: To observe the colors produced when elements are put into a flame and to prove when electrons jump down from higher layers they release energy in the form of light. Materials: CoCl2 Na2SO4 CaCl2 KCl SrCl2 CuCl2 LiCl Unknown A Unknown B Distilled H2O Q-tips Beaker Bunsen Burner Spectroscope Spot Plate Procedure: 1. Light the Bunsen Burner. 2. Fill a beaker with water. 3. Get the spot plate with all the known and unknown salts. 4. Get a Q-tip
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CHEM 1105 Experiment 4: Determination of a Chemical Formula Introduction When atoms of one element combine with those of another‚ the combining ratio is typically an integer or a simple fraction. The simplest formula of a compound expresses that atom ratio. When two or more elements are present in a compound‚ the formula still indicates the atom ratio. To find the formula of a compound we need to find the mass of each of the elements in a weighed sample of that compound. For example‚
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This lab proposed the question of what happens when copper chloride and iron are combined and what is the balanced equation.By completing this lab‚ the goal was to determine the equation and product for the reaction of iron (Fe) and copper chloride (CuCl2). It was predicted either solid iron or solid copper would form. Methods To begin‚ 6.00026 grams of copper chloride was dissolved in 50ml of distilled water in order to have a solution with charged iron and chlorine atoms. Then‚ 6.36 grams of iron
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