Name: strong acids, strong bases, and ph
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 3 min 22 s
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Strong Acid and Base Solutions

חומצות חזקות מתפרקות לגמרי במים. לדוגמה, חומצה חנקתית מתפרקת לחלוטין ליוני הידרוניום וליוני חנקה. מכיוון שיוני ההידורניום שנוצרים מהיינון העצמי של המים הם זניחים, הריכוז של יוני ההידרוניום במים שווה לריכוז של החומצה חזקה.ה-pH בתמיסות אלו ניתן לחישוב באמצעות הריכוז ההתחלתי של החומצה החזקה. לדוגמה, בתמיסת 0.10 מולר HCl, ה-HCl תתפרק לגמרי ליוני הידרוניום ויוני כלוריד, ולכן ריכוז יוני ההידרוניום בתמיסה יהיו 0.10 מולר. על ידי חישוב הלוגריתם השלילי עבור ריכוז זה, ה-pH של התמיסה שווה לאחד.מהצד השני, ניתן להשתמש ב-pH של תמיסה כדי לחשב את ריכוז יוני ההידרוניום בה. לדוגמה, בתמיסה של 3.6 pH, ריכוז יוני ההידרוניום ניתן לחישוב בפתרון המשוואה 3.60 שווה ללוג השלילי של ריכוז יוני ההידרוניום. על מנת לחשב את הריכוז, מכפילים את שני הצדדים במינוס אחד, ומחשבים אנטי לוג לשני הצדדים.ריכוז יוני ההידרוניום שווה ל-2.5 כפול 10 בחזקת מינוס 4 מולר. בסיסים חזקים מהקבוצה הראשונה של מתכות הידרוקסידיות, כמו נתרן הידרוקסידי ואשלגן הידרוקסידי, מתפרקים לגמרי בתמיסה. לדוגמה, נתרן הידרוקסידי 0.20 מולר יתפרק לגמרי במים וייצור 0.20 מולר של יוני נתרן ו-0.20 מולר של יוני הידרוקסיד.אך הקבוצה השנייה של מתכות הידרוקסידיות, כמו בריום הידרוקסידי וסידן הידרוקסידי, מייצרת שני מולים של יוני הידרוקסיד לכל מול של בסיס. לדוגמה, 0.20 מולר של סידן הידרוקסיד יתפרקו לגמרי במים וייצרו 0.020 מולר יוני סידן ו-0.040 מולר יוני הידרוקסיד. אוקסידים של יוני מתכת, כמו נתרן אוקסידי וסידן אוקסידי, גם הם בסיסים חזקים.יון האוקסיד שלהם מגיב עם המים ויוצר יוני הידרוקסיד. ניתן להשתמש בריכוז של יוני הידרוקסיד לחישוב pOH ו-pH בתמיסה. לדוגמה, בתמיסה של אשלגן הידרוקסידי עם 5 כפול 10 בחזקת מינוס 5 מולר יש כמות שווה של יוני הידרוקסיד כבסיס חזק ולכן יש בה pOH של 4.3.כמו ב-pH, ניתן להשתמש ב-pOH של תמיסה לחישוב ריכוז יוני הידרוקסיד על ידי פתרון המשוואה:pOH שווה ללוג שלילי של ריכוז יוני ההידרוקסיד. מכיוון ש-pH ועוד pOH שווים ל-14 ו-pOH הוא 4.3, ה-pH של התמיסה הוא 9.7.

תמיסת חומצות ובסיסים חזקים

<div style="direction:rtl">חומצה חזקה היא תרכובת שמתפרקת לחלוטין בתמיסה מימית ומייצרת ריכוז יוני הידרוניום השווה לריכוז החומצה הראשוני. לדוגמה, חומצה הידברומית של 0.20 M תתפרק לחלוטין במים ותייצר 0.20 M של יוני הידרוניום ו-0.20 M של יוני ברומיד. <img alt="Eq1" src="/files/ftp_upload/11399/11399_Equation_1.png" style="height: 50px;"> מצד שני, בסיס חזק הוא תרכובת שמתפרקת לחלוטין בתמיסה מימית ומייצרת יוני הידרוקסיד. לדוגמה, 0.015 M KOH, הידרוקסיד מתכת קבוצה 1, יתנתק לחלוטין ויפיק 0.015 M של OH- ו-0.015 M שלK+. <img alt="Eq2" src="/files/ftp_upload/11399/11399_Equation_2.png" style="height: 50px;"> 

הידרוקסידים של מתכת מקבוצה 2, כמו בריום הידרוקסיד [Ba(OH)2]וסטרונציום הידרוקסיד [Sr(OH)2], הם גם בסיסים חזקים ויש להם שני יוני הידרוקסיד. זה גורם להם לייצר תמיסה בסיסית יותר בהשוואה ל-NaOH או KOH באותו ריכוז. לדוגמה, 0.015 M Ba(OH)2 מייצר 0.015 M Ba+ ו-0.030 M הידרוקסיד. 

<img alt="Eq3" src="/files/ftp_upload/11399/11399_Equation_3.png" style="height: 50px;"> כאשר חומצות ובסיסים חזקים מתנתקים לחלוטין, ניתן להשתמש ביחסים מולרים כדי לקבוע את ריכוזי ההידרוניום וההידרוקסיד שלהם, אשר בתורם יכולים לשמש לחישוב ה-pH או ה-pOH של תמיסה. לדוגמה, תמיסה של 0.030 M HCl תפיק 0.03 M יוני הידרוניום. לכן ה-pH של תמיסה זו יהיה: <img alt="Eq4" src="/files/ftp_upload/11399/11399_Equation_4.png" style="height: 135px;"> ניתן לקבוע את ה-pOH של אותה תמיסה באמצעות הנוסחה הזו: <img alt="Eq5" src="/files/ftp_upload/11399/11399_Equation_5.png" style="height: 50px;"> מכיוון שה-pH של התמיסה הוא 1.52, ניתן לחשב את ה-pOH שלה כ: <img alt="Eq6" src="/files/ftp_upload/11399/11399_Equation_6.png" style="height: 50px;"> באופן דומה, ניתן להשתמש בריכוז יוני הידרוקסיד המיוצרים על ידי בסיסים חזקים כדי לקבוע את ה-pOH של תמיסה באמצעות המשוואה הזו: <img alt="Eq7" src="/files/ftp_upload/11399/11399_Equation_7.png" style="height: 50px;"> ניתן להשתמש במשוואה לעיל גם כדי לקבוע את ריכוז יוני הידרוקסיד כאשר pOH ידוע. לדוגמה, אם ה-pOH של תמיסה הוא 3.00, <img alt="Eq8" src="/files/ftp_upload/11399/11399_Equation_8.png" style="height: 50px;"> כפל שני הצדדים ב-1 נותן <img alt="Eq9" src="/files/ftp_upload/11399/11399_Equation_9.png" style="height: 50px;"> עכשיו, קח את האנטילוגריתם של שני הצדדים <img alt="Eq10" src="/files/ftp_upload/11399/11399_Equation_10.png" style="height: 90px;"> לפיכך, ריכוז יוני ההידרוניום של התמיסה עם pOH 3 הוא 1.0 × 10−3 M. ניתן להשתמש בשיטה דומה כדי לקבוע את ריכוז יוני ההידרוניום של תמיסה אם ה-pH שלה ידוע.</div>

חומצה חזקה היא תרכובת המתנתקת לחלוטין בתמיסה מימית ומייצרת ריכוז של יוני הידרוניום השווה ל ...

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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

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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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Water as an Amphiprotic Substance

Water can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base. When hydrogen fluoride dissolves in water, it donates protons to water. This is acid ionization. The products are hydronium ions and fluoride ions. Water can also accept protons from another substance. When pyridine dissolves in water, it accepts a proton from water molecules. This is base ionization. The products are hydroxide ions and pyridinium ions. These reactions show that water can play either role. A substance that...

ph scale

pH and pOH in Water

pH and pOH show how hydronium and hydroxide ions behave in water and other aqueous solutions. These ion concentrations are linked by the ion product of water, K w , so when one goes up, the other goes down. Because ion concentrations can differ by huge amounts, a logarithmic scale is used to describe them. pH is defined from the hydronium ion concentration, [H3O+], and pOH is the matching p-function for hydroxide ion concentration. These two values are also connected through the K w...

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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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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...

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acid/base strengths and dissociation constants

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Acid and Base Strength in Water

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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Stepwise Ionization of Polyprotic Acids

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How Bonding Affects Acid Strength

Acid strength depends on bonding, electronegativity, and oxidation number. These factors help explain why some hydrogen compounds act as strong acids, while others behave as weak acids or bases. For binary acids, which are hydrogen compounds with one other nonmetal, acidity increases as the H-A bond gets weaker down a group. That is why the order for group 17 is HF &lt; HCl &lt; HBr &lt; HI, and for group 16 it is H2O &lt; H2S &lt; H2Se &lt; H2Te. Across a period, acid strength increases as...

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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...

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

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Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular ...

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions ...

comparing-intermolecular-forces-melting-point-boiling-point

Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, ...

Construct an explanation to summarize the influences intermolecular forces have on the properties of chemical compounds.

PS.Chm.3.2

Analyze the structure of atoms and isotopes.

Strong Acids, Strong Bases, and pH

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