Name: strong acids, strong bases, and ph
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 3 min 22 s
Channel: JoVE

K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.6.3

Strong Acid and Base Solutions

Kuvvetli asitler suda tamamen ayrışır. Örneğin, nitrik asit tamamen hidronyum iyonlarına ve nitrat iyonlarına ayrışır. Suyun kendiliğinden iyonlaşmasından üretilen hidronyum iyonları ihmal edilebilir düzeyde olduğundan, sudaki hidronyum iyonlarının konsantrasyonu, güçlü asit konsantrasyonuna eşittir.Bu çözeltilerin pH değeri, kuvvetli asidin başlangıç konsantrasyonu kullanılarak belirlenebilir. Örneğin, 0, 10 molar HCl çözeltisinde, HCl, hidronyum iyonlarına ve klorür iyonlarına tamamen ayrışacaktır ve bu nedenle çözeltinin hidronyum iyonu konsantrasyonu da 0, 10 molar olacaktır. Bu konsantrasyonun negatif logaritmasını alındığında, çözeltinin pH değeri bir olarak hesaplanacaktır.Tersine, bir çözeltinin pH'ı bir çözeltinin hidronyum iyon konsantrasyonunu belirlemek için kullanılabilir. Örneğin, pH değeri 3, 60 olan bir çözelti için hidronyum iyon konsantrasyonu, 3, 60, hidronyum iyon konsantrasyonunun negatif loguna eşit olduğu denklemi çözülerek belirlenebilir. Konsantrasyonu çözmek için, her iki tarafı da eksi bir ile çarpın ve ardından her iki tarafın antilogunu alın.Hidronyum iyon konsantrasyonu 2, 5×10⁻⁴ molara eşittir. Sodyum hidroksit ve potasyum hidroksit gibi birinci grup metal hidroksitler olan güçlü bazlar, tamamen çözelti içinde ayrışır. Örneğin 0, 20 molar sodyum hidroksit tamamen suda çözünür ve 0, 20 molar sodyum iyonu ve 0, 20 molar hidroksit iyonu üretir.Bununla birlikte, baryum hidroksit ve kalsiyum hidroksit gibi grup iki metal hidroksit, her bir baz molü için iki mol hidroksit iyonu üretir. Örneğin, 0, 020 molar kalsiyum hidroksit suda tamamen ayrışacak ve 0, 020 molar kalsiyum iyonu 0, 040 molar hidroksit iyonu üretecektir. Sodyum oksit ve kalsiyum oksit gibi iyonik metal oksitler de güçlü bazlardır.Oksit iyonları su ile reaksiyona girer ve hidroksit iyonları üretir. Hidroksit iyonlarının konsantrasyonu, çözeltinin bir pOH ve pH'ını hesaplamak için kullanılabilir. Örneğin, bir 5×10⁻⁵ molar potasyum hidroksit çözeltisi, güçlü baz olarak eşit miktarda hidroksit iyonuna sahiptir ve bu nedenle, 4, 30'luk bir pOH'ye sahiptir.PH gibi, çözeltinin bir pOH'si de denklemi çözerek hidroksit iyon konsantrasyonunu belirlemek için kullanılabilir:pOH, hidroksit iyon konsantrasyonunun negatif loguna eşittir. PH artı pOH 14'e eşit olduğundan ve pOH 4, 3 olduğundan, çözeltinin pH'ı 9, 7'dir.

güçlü asit ve baz Çözeltileri

Güçlü asit, sulu bir çözelti içinde tamamen ayrışan ve başlangıçtaki asit konsantrasyonuna eşit bir konsantrasyonda hidronyum iyonları üreten bir bileşiktir. Örneğin, 0,20 M hidrobromik asit suda tamamen ayrışacak ve 0,20 M hidronyum iyonu ve 0,20 M bromür iyonu üretecektir.
 
 <img alt=""Eq1"" src=""/files/ftp_upload/11399/11399_Equation_1.png"" style=""height: 50px;"" />
 
 Öte yandan, güçlü bir baz, sulu bir çözelti içinde tamamen ayrışan ve hidroksit iyonları üreten bir bileşiktir. Örneğin, bir grup 1 metal hidroksit olan 0,015 M KOH, tamamen ayrışacak ve 0,015 M OH- ve 0,015 M K+ üretecektir.
 
 <img alt=""Eq2"" src=""/files/ftp_upload/11399/11399_Equation_2.png"" style=""height: 50px;"" />
 
 Baryum hidroksit [Ba(OH)2] ve stronsiyum hidroksit [Sr(OH)2] gibi Grup 2 metal hidroksitler de güçlü bazlardır ve iki hidroksit iyonuna sahiptir. Bu, aynı konsantrasyonda NaOH veya KOH ile karşılaştırıldığında daha bazik bir çözelti üretmelerine neden olur. Örneğin, 0,015 M Ba(OH)2  , 0,015 M Ba+  ve 0,030 M hidroksit üretir.
 
 <img alt=""Eq3"" src=""/files/ftp_upload/11399/11399_Equation_3.png"" style=""height: 50px;"" />
 
 Güçlü asitler ve bazlar tamamen ayrıştıkça, molar oranlar, hidronyum ve hidroksit konsantrasyonlarını belirlemek için kullanılabilir ve bu da bir çözeltinin pH’sını veya pOH'sını hesaplamak için kullanılabilir. Örneğin, 0,030 M HCl çözeltisi, 0,03 M hidronyum iyonu üretecektir. Bu nedenle, bu çözeltinin pH'sı aşağıdaki gibi olacaktır.
 
 <img alt=""Eq4"" src=""/files/ftp_upload/11399/11399_Equation_4.png"" style=""height: 135px;"" />
 
 Aynı çözeltinin pOH’sı, aşağıdaki formül kullanılarak belirlenebilir
 
 <img alt=""Eq5"" src=""/files/ftp_upload/11399/11399_Equation_5.png"" style=""height: 50px;"" />
 
 Çözeltinin pH’sı 1,52 olduğu için, onun pOH’sı aşağıdaki gibi hesaplabilir
 
 <img alt=""Eq6"" src=""/files/ftp_upload/11399/11399_Equation_6.png"" style=""height: 50px;"" />
 
 Benzer şekilde, denklemi kullanarak bir çözeltinin pOH'sını belirlemek için güçlü bazlar tarafından üretilen hidroksit iyonlarının konsantrasyonu kullanılabilir.
 
 <img alt=""Eq7"" src=""/files/ftp_upload/11399/11399_Equation_7.png"" style=""height: 50px;"" />
 
 Yukarıdaki denklem, pOH bilindiğinde hidroksit iyon konsantrasyonunu belirlemek için de kullanılabilir. Örneğin, bir çözeltinin pOH'sı 3,00 ise,
 
 <img alt=""Eq8"" src=""/files/ftp_upload/11399/11399_Equation_8.png"" style=""height: 50px;"" />
 
 Her iki tarafında −1 ile çarpılması aşağıdakini verir
 
 <img alt=""Eq9"" src=""/files/ftp_upload/11399/11399_Equation_9.png"" style=""height: 50px;"" />
 
 Şimdi, her iki tarafın anti logaritması alınır
 
 <img alt=""Eq10"" src=""/files/ftp_upload/11399/11399_Equation_10.png"" style=""height: 90px;"" />
 
 Böylece, 3 pOH’ya sahip çözeltinin hidronyum iyon konsantrasyonu 1,0× 10−3 M’dir. pH'sı biliniyorsa, bir çözeltinin hidronyum iyon konsantrasyonunu belirlemek için benzer bir yöntem kullanılabilir.

Güçlü Asit ve Baz Çözeltileri

Güçlü bir asit, sulu bir çözelti içinde tamamen ayrışan ve başlangıçtaki iyona eşit bir hidronyum iyonu konsantrasyonu üreten bir bileşiktir ...

Education

JoVE Core

Kimya

Acids and Bases

Asitler ve Bazlar

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

strong acids, strong bases, and ph

Strong acids and strong bases change the pH of a solution by dissociating completely in water. A strong acid produces hydronium ions, which are H3O+ ions, and a strong base produces hydroxide ions, OH-. Because the dissociation is complete, the ion concentration can be found from the starting concentration and the molar ratio.

For example, 0.20 M hydrobromic acid dissociates fully in water. It produces 0.20 M hydronium ions and 0.20 M bromide ions. A 0.015 M KOH solution also dissociates completely. It produces 0.015 M OH- and 0.015 M K+.

Some group 2 metal hydroxides are also strong bases. Barium hydroxide, Ba(OH)2, and strontium hydroxide, Sr(OH)2, each contain two hydroxide ions. That means they create a more basic solution than NaOH or KOH at the same concentration. For example, 0.015 M Ba(OH)2 produces 0.015 M Ba+ and 0.030 M hydroxide.

The ion concentrations from strong acids and strong bases can be used to calculate pH and pOH. A 0.030 M HCl solution produces 0.03 M hydronium ions, so its pH can be found from that concentration. The same pH value can then be used to determine pOH. If the pH is 1.52, the pOH can be calculated from the relationship between them.

The same idea works for strong bases. The hydroxide ion concentration can be used to find pOH with the equation for pOH, and the equation can also be used in reverse when pOH is known. For example, if the pOH of a solution is 3.00, multiplying by -1 and taking the antilog gives a hydronium ion concentration of 1.0 × 10^-3 M. The same method can be used to find hydronium ion concentration when pH is known.

Strong Acids, Strong Bases, and pH

bronsted-lowry acids and bases

Proton Transfer in Acids and Bases

Acids and bases can be understood through proton transfer. Early scientists described acids by their sour taste, their effect on dyes, and their reaction with limestone, which releases carbon dioxide. Robert Boyle also noted that acid solutions can lose these properties after contact with alkali, or base, solutions. The modern view developed step by step. Humphry Davy showed that hydrogen is the essential part of acids. Joseph Louis Gay-Lussac then described acids as substances that neutralize...

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relative strengths of conjugate acid-base pairs

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How Ka and Kb Show Acid-Base Strength

Brønsted-Lowry acid-base chemistry is based on proton transfer. That idea helps show how the strength of an acid is linked to the strength of its conjugate base, and vice versa. Acid and base strength is measured with ionization constants, Ka and Kb, which tell how far an ionization reaction goes. For the conjugate pair HA and A−, the acid ionizes in water and the base reaction can be written for the partner species. When the two reactions are added, they give the autoionization of water. The...

strong acid and base solutions

Strong acids and strong bases change the pH of a solution by dissociating completely in water. A strong acid produces hydronium ions, which are H3O+ ions, and a strong base produces hydroxide ions, OH-. Because the dissociation is complete, the ion concentration can be found from the starting concentration and the molar ratio. For example, 0.20 M hydrobromic acid dissociates fully in water. It produces 0.20 M hydronium ions and 0.20 M bromide ions. A 0.015 M KOH solution also dissociates...

weak acid solutions

Weak Acid Equilibrium in Water

Weak acid equilibrium in water explains why many acids only partially react when dissolved. Most weak acid molecules stay in their original form, and only a small amount of hydronium ions forms. Weak acids are common in nature. They help create the tangy taste of citrus fruits, the stinging sensation from insect bites, and the smells linked to body odor. Acetic acid is a familiar weak acid. It is the main ingredient in vinegar. Its equation uses a double arrow to show that the reaction with...

weak base solutions

Weak Base pH and Kb Calculations

Weak base pH and Kb calculations show how partially reacting bases change water chemistry. Weak bases produce hydroxide ions when they dissolve by reacting with water molecules. Because the reaction only happens partly, these compounds are classified as weak bases. Weak bases are common in nature and in technology. Ammonia is one major example. Global production of ammonia is typically well over 100 metric tons each year. It is used as an agricultural fertilizer, a starting material for...

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The pH of acid mixtures depends on the acids present, their dissociation constants, and their starting concentrations. When a solution contains two different acids, the pH can be found by choosing the method that fits their relative strengths. This makes acid mixtures a useful case for applying acid-base rules in chemistry. In a mixture of a strong acid and a weak acid, the strong acid dissociates completely and supplies almost all of the hydronium ions in the solution. The weak acid...

ions as acids and bases

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Salt hydrolysis explains why some salt solutions are acidic, basic, or neutral. Salts are ionic compounds made of cations and anions. In water, either ion may react with water through an acid or base ionization reaction. The pH of the solution depends on the relative acid-base strength of the ions in the salt. Ammonium chloride is a good example of an acidic salt. When it dissolves, it separates into ammonium ions and chloride ions. The ammonium ion is the conjugate acid of ammonia, so it can...

determining the ph of salt solutions

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Salt hydrolysis and pH in solutions depend on the ions released when a salt dissolves. Some ions react with water, while others do not. The balance between the cation and anion helps show whether the solution becomes acidic, basic, or neutral. Salts with pH-neutral anions and cations that produce hydronium ions give acidic solutions with pH below 7. Ammonium nitrate is one example. In NH4NO3, NO3− does not react with water, but NH4+ forms hydronium ions, so the solution is acidic. Other salts...

acid/base strengths and dissociation constants

acidbase-strengths-and-dissociation-constants

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Acid and base strength in water depends on how much a substance ionizes after it dissolves. If ionization is nearly complete, the substance is called strong. If only a small amount ionizes, it is called weak. Weak acids and weak bases are much more common than strong ones. The most common strong acids are HClO4, HCl, HBr, HI, HNO3, and H2SO4. The most common strong bases are LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. These strong acids and bases ionize essentially completely in water. <br...

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lewis acids and bases

Electron-Pair Reactions in Acid-Base Chemistry

Electron-pair reactions explain Lewis acid-base chemistry. In 1923, G. N. Lewis described acids and bases by how they accept or donate a pair of electrons. When that electron pair forms a coordinate covalent bond, one atom supplies both bonding electrons. This bond is also called a dative bond. A simple example is the reaction of water with a hydrogen ion to make a hydronium ion. Ammonia can also combine with a hydrogen ion to form an ammonium ion. In both cases, the reaction creates a Lewis...

key terms and concepts

Learn how strong acids and strong bases dissociate completely in water and how their ion concentrations are used to calculate pH and pOH.

Strong Acids, Strong Bases, and pH | JoVE K12

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JoVE Core Kimya, özlü ve kolay anlaşılır animasyon video derslerini kullanarak genel kimya kavramlarına hayat veriyor. Ek olarak, bilim insanı uygulama videolarımız ile klasik ve orijinal araştırma deneylerini dünya çapında günümüz laboratuvarlarında görselleştiriyoruz.

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Ohio’s Learning Standards and Model Curriculum

Interactions Of Matter

Chemical reactions

Minnesota Academic Standards in Science

1.2.1 9L.4.2.2.1

Texas Essential Knowledge and Skills

High School

CHEM.12

CHEM.12.C

Alabama Course of Study Science

Matter and Its Interactions

9-12.C.1.6.a

9-12.PS.3.6.c

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New York State Science Learning Standards

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Strong Acids, Strong Bases, and pH

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