Acids are substances that form hydrogen ions, H+(.pdf

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Acids are substances that form hydrogen ions, H+(aq), when dissolved in water In acid solutions there are more H+ ions than OH- ions. Bases which are soluble in water are called alkalis e.g. NaOH sodium hydroxide, KOH potassium hydroxide or Ca(OH)2 calcium hydroxide. Bases which are water insoluble include CuO copper(II) oxide, MgO magnesium oxide. After a neutralisation, the salt solutions consist of a mixture of positive and negative ions (and their names are in the salt name!) e.g. sodium chloride (NaCl) is a mixture of Na+ and Cl- ions, calcium chloride (CaCl2) is a mix of Ca2+ and Cl- ions; magnesium nitrate (Mg(NO3)2) is a mix of Mg2+ and NO3- ions, aluminium sulphate (Al2(SO4)3) consists of Al3+ and SO42- ions etc. You can test for chloride ions by adding a few drops of dilute nitric acid followed by a few drops of silver nitrate solution. If chloride ions are present you will see a white precipitate of silver chloride. However, chlorine water itself will contain chloride ions as chlorine in aqueous solution disproportionates to form chloride and chlorate(I) ions. Cl2 + H2O --> Cl- + ClO- + 2H+ Testing for the presence of nitrate via wet chemistry is generally difficult compared with testing for other anions, as almost all nitrates are soluble in water. In contrast, many common ions give insoluble salts, e.g. halides precipitate with silver, and sulfates precipitate with barium. The nitrate anion is an oxidizer, and many tests for the nitrate anion are based on this property. Unfortunately, other oxidants present in the analyte may interfere and give erroneous results. Solution Acids are substances that form hydrogen ions, H+(aq), when dissolved in water In acid solutions there are more H+ ions than OH- ions. Bases which are soluble in water are called alkalis e.g. NaOH sodium hydroxide, KOH potassium hydroxide or Ca(OH)2 calcium hydroxide. Bases which are water insoluble include CuO copper(II) oxide, MgO magnesium oxide. After a neutralisation, the salt solutions consist of a mixture of positive and negative ions (and their names are in the salt name!) e.g. sodium chloride (NaCl) is a mixture of Na+ and Cl- ions, calcium chloride (CaCl2) is a mix of Ca2+ and Cl- ions; magnesium nitrate (Mg(NO3)2) is a mix of Mg2+ and NO3- ions, aluminium sulphate (Al2(SO4)3) consists of Al3+ and SO42- ions etc. You can test for chloride ions by adding a few drops of dilute nitric acid followed by a few drops of silver nitrate solution. If chloride ions are present you will see a white precipitate of silver chloride. However, chlorine water itself will contain chloride ions as chlorine in aqueous solution disproportionates to form chloride and chlorate(I) ions. Cl2 + H2O --> Cl- + ClO- + 2H+ Testing for the presence of nitrate via wet chemistry is generally difficult compared with testing for other anions, as almost all nitrates are soluble in water. In contrast, many common ions give insoluble salts, e.g. halides precipitate with silver, and sulfates .

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Unfortunately, other oxidants present in the analyte may interfere and give erroneous results.

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First, let\'s find out what we need. The question asks for the empirical formula of some compound. To do this, we are going to need to find the amount of moles of each substance. To find the moles of Sb, all we will need to do is divide the mass of Sb by the molar mass of Sb. To find the moles of S will be a bit more complicated. Since we know that Sulfur is left over after the reaction, we know that sulfur is in excess (meaning Sb is the only thing that will limit our reaction). Assuming this is an ideal gas, we can take the original amount of moles of Sulfur and subtract it from the moles we get later (after it is transferred to the other container). This will give us the amount of moles of Sulfur that reacted with the moles of Sb. So this is what we need: moles Sb = ? moles S (reacted with Sb) = ? Calculate moles Sb. moles Sb = (mass Sb) / (molar mass Sb) = (0.350g) / (121.76g/mol) = 2.87 x 10^-3 moles Calculate moles S. For this, we are going to have to use the PV = nRT equation two times. One for the S that is placed with the Sb, and one for the S that is placed in the container after the reaction. Moles of S BEFORE reaction: PV = nRT (10.72 atm)(0.100L) = n(0.082)(373.15 K) n = (10.72 atm)(0.100L) / (0.082)(373.15 K) = 0.035 moles S Moles of S AFTER reaction: PV = nRT (14.8 atm)(0.050L) = n(0.082)(323.15 K) n = (14.8 atm)(0.050L) / (0.082)(323.15 K) = 0.028 moles S Calculate moles of S that reacted with the Sb: Since the moles of S went down after the reaction, we know that the moles of S lost must have reacted with the Sb. So, we can simply find the change in moles of S to find the amount of S that reacted with the Sb. Moles of S before reaction - Moles of S after reaction = Moles of S reacted 0.035 moles S - 0.028 moles S = 7.07 x 10^-3 moles S Now that we have our moles of each element that reacted, we can find the empirical formula. To do this, we need to divide through by the element with the least amount of moles. So, in this case, we must divide through by the moles of Sb. (2.87 x 10^-3 moles Sb) / (2.87 x 10^-3 moles Sb) = 1 (7.07 x 10^-3 moles S) / (2.87 x 10^-3 moles Sb) = 2.46 = 2.5 We need subscripts that are integers in empirical formulas. To make 2.5 an integer, we can simply multiply it by 2 to make it 5. When we do this, we also need to multiply 1 by 2. 2.5 x 2 = 5 1 x 2 = 2 These numbers represent the subscripts for each of our elements in our compound. So the empirical formula would be: Sb2S5 Solution First, let\'s find out what we need. The question asks for the empirical formula of some compound. To do this, we are going to need to find the amount of moles of each substance. To find the moles of Sb, all we will need to do is divide the mass of Sb by the molar mass of Sb. To find the moles of S will be a bit more complicated. Since we know that Sulfur is left over after the reaction, we know that sulfur is in excess (meaning Sb is the only thing that will limit our reaction). Assuming this is an ideal gas, we can take.

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Diversity: Diversity scheme refers to a method for improving the reliability of a message signal by using two or more communication channels with different characteristics. Diversity is mainly used in radio communication and is a common technique for combatting fading and co-channel interference and avoiding error bursts. It is based on the fact that individual channels experience different levels of fading and interference. Multiple versions of the same signal may be transmitted and/or received and combined in the receiver Types: In Micro diversity The spacing between transmitters are shorter than wavelength of transmitted signal In Macro diversity The spacing between transmitters are longer than wavelength of transmitted signal Types of microdiversity: Time diversity: Multiple versions of the same signal are transmitted at different time instants. Alternatively, a redundant forward error correction codeis added and the message is spread in time by means of bit-interleaving before it is transmitted. Thus, error bursts are avoided, which simplifies the error correction. Frequency diversity: The signal is transmitted using several frequency channels or spread over a wide spectrum that is affected by frequency-selective fading. Middle-late 20th century microwave radio relay lines often used several regular wideband radio channels, and one protection channel for automatic use by any faded channel. Later examples include: OFDM modulation in combination with subcarrier interleaving and forward error correction Spread spectrum, for example frequency hopping or DS-CDMA. Space diversity: The signal is transmitted over several different propagation paths. In the case of wired transmission, this can be achieved by transmitting via multiple wires. In the case of wireless transmission, it can be achieved by antenna diversity using multiple transmitter antennas (transmit diversity) and/or multiple receiving antennas (reception diversity). In the latter case, a diversity combining technique is applied before further signal processing takes place. If the antennas are far apart, for example at different cellular base station sites or WLAN access points, this is calledmacrodiversity or site diversity. If the antennas are at a distance in the order of one wavelength, this is called microdiversity. A special case is phasedantenna arrays, which also can be used for beamforming, MIMO channels and space–time coding (STC). Polarization diversity: Multiple versions of a signal are transmitted and received via antennas with different polarization. A diversity combiningtechnique is applied on the receiver side. Solution Diversity: Diversity scheme refers to a method for improving the reliability of a message signal by using two or more communication channels with different characteristics. Diversity is mainly used in radio communication and is a common technique for combatting fading and co-channel interference and avoiding error bursts. It is based on the fact that i.

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15.0mL = 0.015L phenylacetic acid 0.50mol/L *0.015= 0.0075 mol phenylacetic acid 20.0mL= 0.020L sodium phenylacetate 0.40mol/L * 0.020L=.008 mol sodium phenylacetate due to the fact that this acts as a buffer Using henderson hasselblach pH= pKa + log(base/acid) and finding that the pKa of phenylaceticacid is 4.28 pH= 4.28 + log (.008/.0075) pH= 4.28 + 0.093 pH= 4.373 Solution 15.0mL = 0.015L phenylacetic acid 0.50mol/L *0.015= 0.0075 mol phenylacetic acid 20.0mL= 0.020L sodium phenylacetate 0.40mol/L * 0.020L=.008 mol sodium phenylacetate due to the fact that this acts as a buffer Using henderson hasselblach pH= pKa + log(base/acid) and finding that the pKa of phenylaceticacid is 4.28 pH= 4.28 + log (.008/.0075) pH= 4.28 + 0.093 pH= 4.373.

15.0mL = 0.015L phenylacetic acid 0.50molL 0.01.pdf

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4: water molecules are like a magnet because because it acts like water 5: As mentioned above, humans have sweat glands over their entire bodies; the only place dogs (and cats, and many other animals with fur over their whole bodies) can get rid of excess heat is through the tongue. By the way, sweating/panting is NOT a means of getting rid of excess water; it is a way of getting rid of heat. We do this because of the process of evaporation. In changing from liquid to vapor, the water absorbs heat from the surface on which it is laying. Actually, most organisms do not want to get rid of excess water; they need to conserve it, but on very hot days animals \"spend\" the water to achieve the cooling. 6. It can dissolve the most types of substances. it can dissolve most substances This is because solutes for the most part are able to dissolve in water with the exception of some solutes like oil. Most of the solids dissolve in water. Solution 4: water molecules are like a magnet because because it acts like water 5: As mentioned above, humans have sweat glands over their entire bodies; the only place dogs (and cats, and many other animals with fur over their whole bodies) can get rid of excess heat is through the tongue. By the way, sweating/panting is NOT a means of getting rid of excess water; it is a way of getting rid of heat. We do this because of the process of evaporation. In changing from liquid to vapor, the water absorbs heat from the surface on which it is laying. Actually, most organisms do not want to get rid of excess water; they need to conserve it, but on very hot days animals \"spend\" the water to achieve the cooling. 6. It can dissolve the most types of substances. it can dissolve most substances This is because solutes for the most part are able to dissolve in water with the exception of some solutes like oil. Most of the solids dissolve in water..

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1. Acids are substances that form hydrogen ions, H+(aq), when dissolved in water In acid solutions there are more H+ ions than OH- ions. Bases which are soluble in water are called alkalis e.g. NaOH sodium hydroxide, KOH potassium hydroxide or Ca(OH)2 calcium hydroxide. Bases which are water insoluble include CuO copper(II) oxide, MgO magnesium oxide. After a neutralisation, the salt solutions consist of a mixture of positive and negative ions (and their names are in the salt name!) e.g. sodium chloride (NaCl) is a mixture of Na+ and Cl- ions, calcium chloride (CaCl2) is a mix of Ca2+ and Cl- ions; magnesium nitrate (Mg(NO3)2) is a mix of Mg2+ and NO3- ions, aluminium sulphate (Al2(SO4)3) consists of Al3+ and SO42- ions etc. You can test for chloride ions by adding a few drops of dilute nitric acid followed by a few drops of silver nitrate solution. If chloride ions are present you will see a white precipitate of silver chloride. However, chlorine water itself will contain chloride ions as chlorine in aqueous solution disproportionates to form chloride and chlorate(I) ions. Cl2 + H2O --> Cl- + ClO- + 2H+ Testing for the presence of nitrate via wet chemistry is generally difficult compared with testing for other anions, as almost all nitrates are soluble in water. In contrast, many common ions give insoluble salts, e.g. halides precipitate with silver, and sulfates precipitate with barium. The nitrate anion is an oxidizer, and many tests for the nitrate anion are based on this property. Unfortunately, other oxidants present in the analyte may interfere and give erroneous results. Solution Acids are substances that form hydrogen ions, H+(aq), when dissolved in water In acid solutions there are more H+ ions than OH- ions. Bases which are soluble in water are called alkalis e.g. NaOH sodium hydroxide, KOH potassium hydroxide or Ca(OH)2 calcium hydroxide. Bases which are water insoluble include CuO copper(II) oxide, MgO magnesium oxide. After a neutralisation, the salt solutions consist of a mixture of positive and negative ions (and their names are in the salt name!) e.g. sodium chloride (NaCl) is a mixture of Na+ and Cl- ions, calcium chloride (CaCl2) is a mix of Ca2+ and Cl- ions; magnesium nitrate (Mg(NO3)2) is a mix of Mg2+ and NO3- ions, aluminium sulphate (Al2(SO4)3) consists of Al3+ and SO42- ions etc. You can test for chloride ions by adding a few drops of dilute nitric acid followed by a few drops of silver nitrate solution. If chloride ions are present you will see a white precipitate of silver chloride. However, chlorine water itself will contain chloride ions as chlorine in aqueous solution disproportionates to form chloride and chlorate(I) ions. Cl2 + H2O --> Cl- + ClO- + 2H+ Testing for the presence of nitrate via wet chemistry is generally difficult compared with testing for other anions, as almost all nitrates are soluble in water. In contrast, many common ions give insoluble salts, e.g. halides precipitate with silver, and sulfates precipitate with barium. The nitrate anion is an oxidizer, and many tests for the nitrate anion are based on this property.

2. Unfortunately, other oxidants present in the analyte may interfere and give erroneous results.

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